Write and balance the equation for the reaction of butane, C 4 H 10 , with oxygen to form carbon dioxide and water. Use your equation to help answer the following questions. (a) Write, in words, a description of the reaction on the particulate level. (b) If you were to build physical ball-and-stick models of the reactants and products, what minimum number of balls representing atoms of each element do you need if you show both reactants and products at the same time? (c) What if the models of the reactants from Part (b) were built and then rearranged to form products? How many balls would you need? (d) Use words to interpret the equation on the molar level. (e) Use the molar-level interpretation of the equation from Part (d) and molar masses rounded to the nearest gram to show that mass is indeed conserved in this reaction.

Question

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Answer 1

Textbook Question

Chapter 8, Problem 8E

Write and balance the equation for the reaction of butane, $C 4 H 10$ , with oxygen to form carbon dioxide and water. Use your equation to help answer the following questions. (a) Write, in words, a description of the reaction on the particulate level. (b) If you were to build physical ball-and-stick models of the reactants and products, what minimum number of balls representing atoms of each element do you need if you show both reactants and products at the same time? (c) What if the models of the reactants from Part (b) were built and then rearranged to form products? How many balls would you need? (d) Use words to interpret the equation on the molar level. (e) Use the molar-level interpretation of the equation from Part (d) and molar masses rounded to the nearest gram to show that mass is indeed conserved in this reaction.

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

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Answer 2

Textbook Question

Chapter 8, Problem 8E

Write and balance the equation for the reaction of butane, $C 4 H 10$ , with oxygen to form carbon dioxide and water. Use your equation to help answer the following questions. (a) Write, in words, a description of the reaction on the particulate level. (b) If you were to build physical ball-and-stick models of the reactants and products, what minimum number of balls representing atoms of each element do you need if you show both reactants and products at the same time? (c) What if the models of the reactants from Part (b) were built and then rearranged to form products? How many balls would you need? (d) Use words to interpret the equation on the molar level. (e) Use the molar-level interpretation of the equation from Part (d) and molar masses rounded to the nearest gram to show that mass is indeed conserved in this reaction.

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

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Answer 3

Textbook Question

Chapter 8, Problem 8E

Write and balance the equation for the reaction of butane, $C 4 H 10$ , with oxygen to form carbon dioxide and water. Use your equation to help answer the following questions. (a) Write, in words, a description of the reaction on the particulate level. (b) If you were to build physical ball-and-stick models of the reactants and products, what minimum number of balls representing atoms of each element do you need if you show both reactants and products at the same time? (c) What if the models of the reactants from Part (b) were built and then rearranged to form products? How many balls would you need? (d) Use words to interpret the equation on the molar level. (e) Use the molar-level interpretation of the equation from Part (d) and molar masses rounded to the nearest gram to show that mass is indeed conserved in this reaction.

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

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Answer 4

Textbook Question

Chapter 8, Problem 8E

Write and balance the equation for the reaction of butane, $C 4 H 10$ , with oxygen to form carbon dioxide and water. Use your equation to help answer the following questions. (a) Write, in words, a description of the reaction on the particulate level. (b) If you were to build physical ball-and-stick models of the reactants and products, what minimum number of balls representing atoms of each element do you need if you show both reactants and products at the same time? (c) What if the models of the reactants from Part (b) were built and then rearranged to form products? How many balls would you need? (d) Use words to interpret the equation on the molar level. (e) Use the molar-level interpretation of the equation from Part (d) and molar masses rounded to the nearest gram to show that mass is indeed conserved in this reaction.

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

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Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Answer 8

Expert Solution

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Interpretation Introduction

(a)

Interpretation:

The description of the given reaction is to be stated on the particulate level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer 13

Answer to Problem 8E

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Answer 14

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecules of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Answer 15

Conclusion

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

Answer 16

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Expert Solution

Answer 20

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer 21

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Answer 22

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms, oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule, two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule, two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation, reactant requires, $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms, whereas products require $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms. In total $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms are required.

Answer 23

Conclusion

The minimum number of balls representing atoms of each element required to show both reactants and products at the same time are $16$ carbon atoms, $40$ hydrogen atoms and $52$ oxygen atoms.

Answer 24

Expert Solution

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Answer 25

Expert Solution

Answer 26

Expert Solution

Answer 27

Expert Solution

Answer 28

Interpretation Introduction

(b)

Interpretation:

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer 29

Answer to Problem 8E

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Answer 30

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

The reaction is multiplied by factor of $2$ and thus, the reaction becomes,

$2C4H10(l)+13O2(g)→8CO2(g)+10H2O(g)$

At particulate level, two molecule of butane reacts with thirteen molecules of oxygen to form eight molecules of carbon dioxide and ten molecules of water.

In reactants, for one molecule of butane, four atoms of carbon and ten atoms of hydrogen is required and for oxygen molecule two atoms of oxygen are required.

In products, for one molecule of carbon dioxide, one atom of carbon and two atoms of oxygen are required and for water molecule two atoms of hydrogen and one atom of oxygen are required.

To depict the given balanced equation reactant requires, $8$ carbon atoms, $20$ hydrogen atoms, $26$ oxygen atoms. The numbers of atoms are balanced on both the sides of the reaction. Thus, in total $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms are required.

Answer 31

Conclusion

The minimum number of balls representing atoms of each element required to show reactants which are then rearranged to products are $8$ carbon atoms, $20$ hydrogen atoms and $26$ oxygen atoms.

Answer 32

Expert Solution

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Answer 33

Expert Solution

Answer 34

Expert Solution

Answer 35

Expert Solution

Answer 36

Interpretation Introduction

(d)

Interpretation:

The description of the given reaction is to be stated on the molar level.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer 37

Answer to Problem 8E

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Answer 38

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Answer 39

Conclusion

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

Answer 40

Expert Solution

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.

At molar level, one mole of butane reacts with $132$ moles of oxygen to form four moles of carbon dioxide and five moles of water.

The molar mass of carbon is $12.01 g/mol$ .

The molar mass of hydrogen is $1.008 g/mol$ .

The molar mass of oxygen is $16.00 g/mol$ .

The mass of reactants is calculated by the sum of mass of each reactant.

The molar mass of butane is calculated as follows,

$Molar mass of butane=(4×Molar mass of carbon+10×Molar mass of hydrogen)$

Substitute the molar mass of carbon and hydrogen in the above formula.

$Molar mass of butane=(4×12 g/mol+10×1 g/mol)Molar mass of butane=(48 g/mol+10 g/mol)Molar mass of butane=58 g/mol$

The molar mass of oxygen is calculated as follows,

$Molar mass of oxygen=2×Molar mass of oxygen$

Substitute the molar mass of oxygen in the above formula.

$Molar mass of oxygen=2×16 g/molMolar mass of oxygen=32 g/mol$

The total mass of oxygen is,

$Mass of oxygen=6.5 mol×32 g/molMass of oxygen=208 g$

Total mass of reactants is $208 g+58 g=266 g$ .

The molar mass of carbon dioxide is calculated as follows,

$Molar mass of carbon dioxide=(1×Molar mass of carbon+2×Molar mass of oxygen)$

Substitute the molar mass of carbon and oxygen in the above formula.

$Molar mass of carbon dioxide=(1×12 g/mol+2×16 g/mol)Molar mass of carbon dioxide=(12 g/mol+32 g/mol)Molar mass of carbon dioxide=44 g/mol$

The molar mass of water is calculated as follows,

$Molar mass of water=1×Molar mass of oxygen+2×Molar mass of hydrogen$

Substitute the molar mass of oxygen and hydrogen in the above formula.

$Molar mass of water=1×16 g/mol+2×1 g/molMolar mass of water=18 g/mol$

The total mass of carbon dioxide is,

$Mass of carbon dioxide=4 mol×44 g/molMass of carbon dioxide=176 g$

The total mass of water is,

$Mass of water=5 mol×18 g/molMass of water=90 g$

Total mass of products is $176 g+90 g=266 g$ .

The mass of reactants and products is same, thus, the mass is conserved.

Conclusion

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Answer 41

Expert Solution

Answer 42

Expert Solution

Answer 43

Expert Solution

Answer 44

Interpretation Introduction

(e)

Interpretation:

The validation of the fact that the mass is conserved for the given reaction is to be stated.

Concept introduction:

In a balanced chemical equation, all the reactants and products are written with their stoichiometric coefficients and their physical states. The number of atoms of an element on both sides of a balanced chemical equation is equal.

Answer 45

Answer to Problem 8E

The mass of reactants and products is same and thus, the mass of the given reaction is conserved.

Answer 46

Explanation of Solution

The butane undergoes combustion reaction in presence of oxygen to form carbon dioxide and water. The corresponding chemical reaction is,

$C4H10(l)+O2(g)→CO2(g)+H2O(g)$

To balance the given chemical equation, the number of carbon atoms, oxygen atoms, and hydrogen atoms should be same on both the sides. The balanced chemical equation is,

$C4H10(l)+132O2(g)→4CO2(g)+5H2O(g)$

To balance the number of carbon atoms oxygen atoms, and hydrogen atoms, the coefficient of $4$ is placed before carbon dioxide, the coefficient of $5$ is placed before water and the coefficient of $132$ is placed before oxygen gas.