CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<
CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<
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ISBN: 9780357096949
Author: Kotz
Publisher: CENGAGE C
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Chapter 5, Problem 111SCQ

Isomers are molecules with the same elemental composition but a different atomic arrangement. Three isomers with the formula C4H8 are shown in the models below. The enthalpy of combustion (ΔcH°) of each isomer, determined using a calorimeter, is as follows:

Chapter 5, Problem 111SCQ, Isomers are molecules with the same elemental composition but a different atomic arrangement. Three

  1. (a) Draw an energy level diagram relating the energy content of the three isomers to the energy content of the combustion products, CO2(g) and H2O().
  2. (b) Use the ΔcH° data in part (a), along with the enthalpies of formation of CO2(g) and H2O() from Appendix L, to calculate the enthalpy of formation for each of the isomers.
  3. (c) Draw an energy level diagram that relates the enthalpies of formation of the three isomers to the energy of the elements in their standard states.
  4. (d) What is the enthalpy change for the conversion of cis-2-butene to trans-2-butene?

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The energy level diagram relating the energy content of the three isomers has to be determined

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity,ΔT= change in temperature.

The standard molar enthalpy of formation is the enthalpy change ΔfH0 is the enthalpy change for the formation of 1mol a compound directly from its component elements in their standard states. And is given by

  ΔrH0CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  1ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation of Solution

The energy level diagram is given below

CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  2

Figure 1

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The enthalpy of formation of CO2andH2O has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g substance by 1K.Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity,ΔT= change in temperature.

The standard molar enthalpy of formation is the enthalpy change ΔfH0 is the enthalpy change for the formation of 1mol of a compound directly from its component elements in their standard states. And is given by

  ΔrH0CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  3ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation of Solution

Given reaction is:

  C4H8+6O24CO2+4H2O

For cis-2-butene

Using the formula ΔrH0CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  4ΣnΔfH0(products)-ΣnΔfH0(reactants)

(1mol×-2709.8kJ/mol)=(4mol×-393.5kJ/mol)+(4mol×-285.83kJ/mol)-(1mol×ΔfH0C4H8)-2709.8=-2717.40-ΔfH0C4H8ΔfH0C4H8=-2717.40-(-2709.8)=-7.6kJ/mol

For trans-2-butene

Using the formula ΔrH0CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  5ΣnΔfH0(products)-ΣnΔfH0(reactants)

(1mol×-2706.6kJ/mol)=(4mol×-393.5kJ/mol)+(4mol×-285.83kJ/mol)-(1mol×ΔfH0C4H8)-2706.6=-2717.40-ΔfH0C4H8ΔfH0C4H8=-2717.40-(-2706.6)=10.8kJ/mol

ΔfH0C4H8=10.8kJ/mol

For 1-butene

Using the formula ΔrH0CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  6ΣnΔfH0(products)-ΣnΔfH0(reactants)

(1mol×-2716.8kJ/mol)=(4mol×-393.5kJ/mol)+(4mol×-285.83kJ/mol)-(1mol×ΔfH0C4H8)-2716.8=-2717.40-ΔfH0C4H8ΔfH0C4H8=-2717.40-(-2716.8)=0.6kJ/mol

ΔfH0C4H8=0.6kJ/mol

the enthalpy of formation for each of the isomers found out.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The energy level diagram based on the enthalpy of formation has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, ΔT= change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

  ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation of Solution

The energy level diagram based on the enthalpy of formation is:

  CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<, Chapter 5, Problem 111SCQ , additional homework tip  7

     Figure 2

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The enthalpy change for the conversion of cis-2-butene to trans-2-butene has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K. Energy gained or lost can be calculated using the below equation.

  q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, ΔT= change in temperature.

The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one gram of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

  ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation of Solution

Form the question the values given are:

cis-2-buteneΔH(kJ/mol)=-2709.8trans-2-buteneΔH(kJ/mol)=-2706.6

Enthalpy change of cis-2-butence to trans-2-butene

ΔrH0=ΔfH0 (trans-2-butene) - ΔfH0(cis-2-butence)

ΔrH0=-2706.6kJ/mol-(-2709.8kJ/mol)=-3.3kJ/mol

ΔrH0=-3.3kJ/mol

So, the enthalpy change for a conversion of cis-2-butence to trans-2-butene is

ΔrH0=-3.3kJ/mol

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Chapter 5 Solutions

CHEMISTRY+CHEM...(LL)-W/ACCESS >CUSTOM<

Ch. 5.8 - The standard enthalpies of formation of KNO3(s)...Ch. 5.8 - Prob. 1.2ACPCh. 5.8 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.8 - Prob. 2.1ACPCh. 5.8 - Prob. 2.2ACPCh. 5.8 - Prob. 2.3ACPCh. 5.8 - Prob. 2.4ACPCh. 5.8 - Prob. 2.5ACPCh. 5 - Define the terms system and surroundings. What...Ch. 5 - What determines the directionality of energy...Ch. 5 - Identify whether the following processes are...Ch. 5 - Identify whether the following processes are...Ch. 5 - The molar heat capacity of mercury is 28.1 J/mol ...Ch. 5 - The specific heat capacity of benzene (C6H6) is...Ch. 5 - The specific heat capacity of copper metal is...Ch. 5 - How much energy as heat is required to raise the...Ch. 5 - The initial temperature of a 344-g sample of iron...Ch. 5 - After absorbing 1.850 kJ of energy as heat, the...Ch. 5 - A 45.5-g sample of copper at 99.8 C is dropped...Ch. 5 - One beaker contains 156 g of water at 22 C, and a...Ch. 5 - A 182-g sample of gold at some temperature was...Ch. 5 - When 108 g of water at a temperature of 22.5 C is...Ch. 5 - A 13.8-g piece of zinc is heated to 98.8 C in...Ch. 5 - A 237-g piece of molybdenum, initially at 100.0 C,...Ch. 5 - How much energy is evolved as heat when 1.0 L of...Ch. 5 - The energy required to melt 1.00 g of ice at 0 C...Ch. 5 - How much energy is required to vaporize 125 g of...Ch. 5 - Chloromethane, CH3CI, arises from microbial...Ch. 5 - The freezing point of mercury is 38.8 C. 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CH3CO2H, is made industrially by the...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - A piece of titanium metal with a mass of 20.8 g is...Ch. 5 - A piece of chromium metal with a mass of 24.26 g...Ch. 5 - Adding 5.44 g of NH4NO3(s) to 150.0 g of water in...Ch. 5 - You should use care when dissolving H2SO4 in water...Ch. 5 - Sulfur (2.56 g) was burned in a constant-volume...Ch. 5 - Suppose you burned 0.300 g of C(s) in an excess of...Ch. 5 - Suppose you burned 1.500 g of benzoic acid,...Ch. 5 - A 0.692-g sample of glucose, C6H12O6, was burned...Ch. 5 - An ice calorimeter can be used to determine the...Ch. 5 - A 9.36-g piece of platinum was heated to 98.6 C in...Ch. 5 - The enthalpy changes for the following reactions...Ch. 5 - The enthalpy changes of the following reactions...Ch. 5 - Enthalpy changes for the following reactions can...Ch. 5 - You wish to know the enthalpy change for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - The first step in the production of nitric acid...Ch. 5 - The Romans used calcium oxide, CaO, to produce a...Ch. 5 - The standard enthalpy of formation of solid barium...Ch. 5 - An important step in the production of sulfuric...Ch. 5 - The enthalpy change for the oxidation of...Ch. 5 - The enthalpy change for the oxidation of styrene....Ch. 5 - Prob. 65GQCh. 5 - Prob. 66GQCh. 5 - For each of the following, define a system and its...Ch. 5 - Prob. 68GQCh. 5 - Use Appendix L to find the standard enthalpies of...Ch. 5 - You have a large balloon containing 1.0 mol of...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Use standard enthalpies of formation to calculate...Ch. 5 - Which evolves more energy on cooling from 50 C to...Ch. 5 - You determine that 187 J of energy as heat is...Ch. 5 - Calculate the quantity of energy required to...Ch. 5 - You add 100.0 g of water at 60.0 C to 100.0 g of...Ch. 5 - Three 45-g ice cubes at 0 C are dropped into 5.00 ...Ch. 5 - Suppose that only two 45-g ice cubes had been...Ch. 5 - You take a diet cola from the refrigerator and...Ch. 5 - The standard molar enthalpy of formation of...Ch. 5 - Chloromethane, CH3Cl, a compound found throughout...Ch. 5 - Prob. 83GQCh. 5 - Camping stoves are fueled by propane (C3H8),...Ch. 5 - Prob. 85GQCh. 5 - Prob. 86GQCh. 5 - (a) Calculate the enthalpy change, rH, for the...Ch. 5 - You drink 350 mL of diet soda that is at a...Ch. 5 - Chloroform, CHCl3, is formed from methane and...Ch. 5 - Water gas, a mixture of carbon monoxide and...Ch. 5 - Using standard enthalpies of formation, verify...Ch. 5 - A piece of lead with a mass of 27.3 g was heated...Ch. 5 - A 192-g piece of copper is heated to 100.0 C in a...Ch. 5 - Insoluble AgCl(s) precipitates when solutions of...Ch. 5 - Insoluble PbBr2(s) precipitates when solutions of...Ch. 5 - The value of U for the decomposition of 7.647 g of...Ch. 5 - A bomb calorimetric experiment was run to...Ch. 5 - The meals-ready-to-eat (MREs) in the military can...Ch. 5 - On a cold day, you can warm your hands with a heat...Ch. 5 - Without doing calculations, decide whether each of...Ch. 5 - Prob. 102SCQCh. 5 - You want to determine the value for the enthalpy...Ch. 5 - Prepare a graph of specific heat capacities for...Ch. 5 - Prob. 105SCQCh. 5 - You are attending summer school and living in a...Ch. 5 - Prob. 107SCQCh. 5 - Prob. 108SCQCh. 5 - Prob. 109SCQCh. 5 - Peanuts and peanut oil are organic materials and...Ch. 5 - Isomers are molecules with the same elemental...Ch. 5 - Prob. 112SCQCh. 5 - Prob. 113SCQCh. 5 - A piece of gold (10.0 g, CAu = 0.129 J/g K) is...Ch. 5 - Methane, CH4, can be converted to methanol, which,...Ch. 5 - Calculate rH for the reaction 2 C(s) + 3 H2(g) + ...Ch. 5 - You have the six pieces of metal listed below,...Ch. 5 - Sublimation of 1.0 g of dry ice. CO2(s), forms...Ch. 5 - In the reaction of two moles of gaseous hydrogen...
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