
(a)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of oxidation-reduction reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of oxidation −reduction reaction because in the above reaction oxidation number changed.
(b)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of oxidation-reduction reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of oxidation −reduction reaction because in the above reaction oxidation number changed.
(c)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of acid -base reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of acid −base or neutralization reaction because here salt and water will form.
(d)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of acid -base reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of acid −base or neutralization reaction because here salt and water will form.
(e)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of precipitation reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of precipitation reaction because here a solid
(f)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of precipitation reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of precipitation reaction because here a solid
(g)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of oxidation-reduction reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of oxidation −reduction reaction because in the above reaction oxidation number changed.
(h)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of oxidation-reduction reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of oxidation −reduction reaction because in the above reaction oxidation number changed.
(i)
Interpretation:
To complete and balance the given combustion reaction.
Concept Introduction:
A balanced chemical equation is an equation that contains same number of atoms as well as of each element of reactants and products of reaction.
For example, the reaction between lead sulphide and oxygen is as follows:
Oxidation-reduction reaction is known as redox reaction. In these types of reaction one reactant is oxidized and another is reduced.
Oxidation: Oxidation is a process in which either 1 or all following changes occurs:
- Gaining of oxygen atoms.
- Loss of electrons.
- Loss of hydrogen atom.
Reduction: Reduction is a process in which either 1 or all following changes occurs:
- Loss of oxygen atoms.
- Gaining of electrons.
- Gaining of hydrogen atom.
Precipitation reaction means formation of solids or formation of any Precipitate; when solutions of two ionic substances are mixed and any solid will forms in the solution mixture, the reaction is known as Precipitation reaction. The reaction of barium hydroxide and sodium sulphate is an example of precipitate reaction, where barium sulphate a precipitate is formed as follows:
When an acid is reacted with base creating water or solvent and an ionic salt, the reaction is known as Acid-base neutralization reaction for example the reaction of strong acid, hydrochloric acid with strong base sodium hydroxide is as follows:

Answer to Problem 54QAP
The given reaction is an example of acid -base reaction.
Explanation of Solution
Given:
The balance reaction is as follows:
This is an example of acid −base or neutralization reaction because here salt and water will form.
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Chapter 7 Solutions
Introductory Chemistry: A Foundation
- Using reaction free energy to predict equilibrium composition Consider the following equilibrium: N2 (g) + 3H2 (g) = 2NH3 (g) AG⁰ = -34. KJ Now suppose a reaction vessel is filled with 8.06 atm of nitrogen (N2) and 2.58 atm of ammonia (NH3) at 106. °C. Answer the following questions about this system: ? rise Under these conditions, will the pressure of N2 tend to rise or fall? ☐ x10 fall Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N2 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N2 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm ☑ 5 00. 18 Ararrow_forwardi need help with the followingarrow_forwardUsing reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NO(g) +Cl₂ (g) = 2NOC1 (g) AGº = -41. kJ Now suppose a reaction vessel is filled with 8.90 atm of chlorine (C12) and 5.71 atm of nitrosyl chloride (NOC1) at 1075. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCI tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. atm ☑ 18 Ararrow_forward
- Identifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. acids: 0.29 mol of NaOH is added to 1.0 L of a 1.2M HCN solution. bases: ☑ other: 0.09 mol of HCl is added to acids: 1.0 L of a solution that is bases: 0.3M in both HCN and KCN. other: 0,0,... ? 00. 18 Ar 日arrow_forwardIdentifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. acids: 0.2 mol of KOH is added to 1.0 L of a 0.5 M HF solution. bases: Х other: ☐ acids: 0.10 mol of HI is added to 1.0 L of a solution that is 1.4M in both HF and NaF. bases: other: ☐ 0,0,... ด ? 18 Ararrow_forwardIdentifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. acids: ☐ 1.8 mol of HCl is added to 1.0 L of a 1.0M NH3 bases: ☐ solution. other: ☐ 0.18 mol of HNO3 is added to 1.0 L of a solution that is 1.4M in both NH3 and NH₁Br. acids: bases: ☐ other: ☐ 0,0,... ? 000 18 Ar B 1arrow_forward
- Using reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NH3 (g) = N2 (g) +3H₂ —N2 (g) AGº = 34. kJ Now suppose a reaction vessel is filled with 4.19 atm of ammonia (NH3) and 9.94 atm of nitrogen (N2) at 378. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH 3 tend to rise or fall? ☐ x10 fall Х Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH 3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no atm 00. 18 Ar 무ㅎ ?arrow_forwardIdentifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. 2.2 mol of NaOH is added to 1.0 L of a 1.4M HF solution. acids: П bases: Х other: ☐ ப acids: 0.51 mol of KOH is added to 1.0 L of a solution that is bases: 1.3M in both HF and NaF. other: ☐ 00. 18 Ararrow_forwardUsing reaction free energy to predict equilibrium composition Consider the following equilibrium: N2O4 (g) 2NO2 (g) AG⁰ = 5.4 kJ Now suppose a reaction vessel is filled with 1.68 atm of dinitrogen tetroxide (N204) at 148. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N2O4 tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO 2 needed to reverse it. Round your answer to 2 significant digits. yes no 0.42 atm ☑ 5 0/5 ? مله Ararrow_forward
- Homework 13 (Ch17) Question 4 of 4 (1 point) | Question Attempt: 2 of 2 ✓ 1 ✓ 2 = 3 4 Time Remaining: 4:25:54 Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction: 2CH3OH (g)+302 (g) → 2CO2 (g) + 4H₂O (g) Round your answer to zero decimal places. ☐ kJ x10 ☐ Subm Check 2020 Hill LLC. All Rights Reserved. Terms of Use | Privacy Cearrow_forwardIdentifying the major species in weak acid or weak base equilibria Your answer is incorrect. • Row 2: Your answer is incorrect. • Row 3: Your answer is incorrect. • Row 6: Your answer is incorrect. 0/5 The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. acids: HF 0.1 mol of NaOH is added to 1.0 L of a 0.7M HF solution. bases: 0.13 mol of HCl is added to 1.0 L of a solution that is 1.0M in both HF and KF. Exponent other: F acids: HF bases: F other: K 1 0,0,... ? 000 18 Ararrow_forwardUsing reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NOCI (g) 2NO (g) + Cl2 (g) AGº =41. kJ Now suppose a reaction vessel is filled with 4.50 atm of nitrosyl chloride (NOCI) and 6.38 atm of chlorine (C12) at 212. °C. Answer the following questions about this system: ? rise Under these conditions, will the pressure of NOCI tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. 0.035 atm ✓ G 00. 18 Ararrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning

