Student Solutions Manual for Ball's Physical Chemistry, 2nd
Student Solutions Manual for Ball's Physical Chemistry, 2nd
2nd Edition
ISBN: 9798214169019
Author: David W. Ball
Publisher: Cengage Learning US
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 8, Problem 8.14E
Interpretation Introduction

Interpretation:

The reaction that can provide 5.00×102 kJ of work is to be identified.

Concept Introduction:

Standard Gibbs free energy of a reaction is used check whether the reaction is spontaneous or not. If the value of ΔG° is positive, then the reaction is non spontaneous. If the value of ΔG° is negative, then the reaction is spontaneous. Standard Gibbs free energy of a redox reaction is also represented as the maximum amount of work done by the system on the surroundings.

Expert Solution & Answer
Check Mark

Answer to Problem 8.14E

Correct answer:

The correct option is (b).

Explanation of Solution

Reason for correct answer:

(b)

The given chemical equation (b) is represented as,

Ca(s)+H+Ca2++H2

From Table 8.2, the reduction half reaction of Ca2+ and the standard reduction potential of Ca2+ is represented as,

Ca2++2eCa      E°=2.868V

The above equation is reversed and the value of E° is multiplied by 1., to form an oxidation half reaction. The oxidation half reaction is represented as,

CaCa2++2e      E°=2.868V …(1)

The number of moles of electrons transferred in the above reaction is 2mol.

From Table 8.2, the reduction half reaction of H+ and the standard reduction potential of H+ is represented as,

2H++2eH2     E°=0V …(2)

The number of moles of electrons transferred in the above reaction is 2mol.

The relation between standard Gibbs free energy and standard electrical potential is represented as,

ΔG°=nFE° …(3)

Where,

ΔG° represents the standard Gibbs free energy of the reaction.

N represents the number of moles.

F represents the Faraday’s constant with value 96,485 C/mol.

E° represents the standard electrical potential.

Substitute the values of the standard oxidation potential of Ca, F and number of moles of electrons transferred in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(2.868V)(1J/C1 V)=(553437.96J)(1 kJ1000 J)=553.438kJ

The value ΔG° for the reaction (1) is 553.438kJ.

The standard electrical potential of the reaction (2) is 0.0V. Therefore, the value ΔG° for the reaction (2) is 0 kJ.

The balanced overall electron chemical reaction is obtained when chemical equation (1) is added in chemical equation (2). The formation of overall balanced chemical equation is represented as,

CaCa2++2e                ΔG°=553.438kJ2H++2eH2                ΔG°=0kJCa(s)+2H+Ca2++H2ΔG°=553.438kJ

Therefore, the value ΔG° for the given reaction is 553.438kJ.

The maximum amount of work that can be done by the given chemical reaction (b) is 553.438kJ.

The required work done is 5.00×102 kJ.

Therefore, the given reaction (b) can provide enough energy to perform the process.

The correct option is (b).

Reason for incorrect options:

(a)

The given chemical equation (a) is represented as,

Zn(s)+Cu2+Zn2++Cu(s)

From Table 8.2, the reduction half reaction of Zn2+ and the standard reduction potential of Zn2+ is represented as,

Zn2++2eZn      E°=0.7618V

The above equation is reversed and the value of E° is multiplied by 1, to form an oxidation half reaction. The oxidation half reaction is represented as,

ZnZn2++2e      E°=0.7618V …(4)

The number of moles of electrons transfer in the above reaction is 2mol.

From Table 8.2, the reduction half reaction of Cu+ and the standard reduction potential of Cu+ is represented as,

Cu2++2eCu     E°=0.3419V …(5)

The number of moles of electrons transferred in the above reaction is 2mol.

Substitute the values of the standard oxidation potential of Zn, F and number of moles of electrons transfer in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(0.7618V)(1J/C1 V)=(147004.546J)(1 kJ1000 J)=147.004kJ

The value ΔG° for the reaction (4) is 147.004kJ.

Substitute the values of the standard reduction potential of Cu, F and number of moles of electrons transfer in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(0.3419V)(1J/C1 V)=(65976.443J)(1 kJ1000 J)=65.9764kJ

The value ΔG° for the reaction (5) is 65.9764kJ.

The balanced overall electron chemical reaction is obtained when chemical equation (4) is added in chemical equation (5). The formation of overall balanced chemical equation is represented as,

ZnZn2++2e                       ΔG°=147.004kJCu2++2eCu                       ΔG°=65.9764kJZn(s)+Cu2+Zn2++Cu(s)ΔG°=212.9804kJ

Therefore, the value ΔG° for the given reaction (a) is 212.9804kJ.

(c)

The given chemical equation (c) is represented as,

Li(s)+H2OLi++H2+OH

From Table 8.2, the reduction half reaction of Li+ and the standard reduction potential of Li+ is represented as,

Li++eLi      E°=3.04V

The above equation is reversed and the value of E° is multiplied by 1, to from an oxidation half reaction. The oxidation half reaction is represented as,

LiLi++e      E°=3.04V …(6)

The number of moles of electrons transfer in the above reaction is 1mol.

From Table 8.2, the reduction half reaction of H2O and the standard reduction potential of H2O is represented as,

2H2O+2eH2+2OH     E°=0.8277V …(7)

The number of moles of electrons transfer in the above reaction is 2mol.

Substitute the values of the standard oxidation potential of Li, F and number of moles of electrons transfer in the equation (3).

ΔG°=(1 mol)(96,485 C/mol)(3.04V)(1J/C1 V)=(293314.4J)(1 kJ1000 J)=293.3144kJ

The value ΔG° for the reaction (6) is 293.3144kJ.

Substitute the values of the standard reduction potential of H2O, F and number of moles of electrons transfer in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(0.8277V)(1J/C1 V)=(159721.269J)(1 kJ1000 J)=159.721kJ

The value ΔG° for the reaction (7) is 159.721kJ.

The balanced overall electron chemical reaction is obtained when chemical equation (6) is multiplied by 2 and then added in chemical equation (7). The formation of overall balanced chemical equation is represented as,

2Li2Li++2e                                 2×ΔG°=2×(293.3144kJ)2H2O+2eH2+2OH                         ΔG°=159.721kJ2Li(s)+2H2O2Li++2OH+H2       ΔG°=426.9078kJ

Therefore, the value ΔG° for the given reaction (c) is 426.9078kJ.

(d)

The given chemical equation (d) is represented as,

H2+OH+Hg2Cl2H2O+Hg+Cl

From Table 8.2, the reduction half reaction of Hg2Cl2 and the standard reduction potential of Hg2Cl2 is represented as,

Hg2Cl2+2e2Hg+2Cl         E°=0.2682V …(8)

The number of moles of electrons transferred in the above reaction is 2mol.

The chemical equation (7) is reversed and the value of E° is multiplied by 1, to from an oxidation half reaction. The oxidation half reaction is represented as,

H2+2OH2H2O+2e    E°=0.8277V …(9)

The number of moles of electrons transferred in the above reaction is 2mol.

Substitute the values of the standard reduction potential of Hg2Cl2, F and number of moles of electrons transfer in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(0.2682V)(1J/C1 V)=(51754.554J)(1 kJ1000 J)=51.7546kJ

The value ΔG° for the reaction (8) is 51.7546kJ.

Substitute the values of the standard oxidation potential of H2O, F and number of moles of electrons transferred in the equation (3).

ΔG°=(2 mol)(96,485 C/mol)(0.8277V)(1J/C1 V)=(159721.269J)(1 kJ1000 J)=159.721kJ

The value ΔG° for the reaction (7) is 159.721kJ.

The balanced overall electron chemical reaction is obtained when chemical equation (6) is added in chemical equation (7). The formation of overall balanced chemical equation is represented as,

Hg2Cl2+2e2Hg+2Cl                           ΔG°=51.7546kJH2+2OH2H2O+2e                               ΔG°=159.721kJH2+2OH+Hg2Cl22H2O+2Hg+Cl    ΔG°=211.4756kJ

The value ΔG° for the given reaction (d) is 211.4756kJ.

Therefore, the option (a), (c) and (d) are incorrect.

Conclusion

The reaction (b) provides sufficient amount of energy to do required work. Therefore, the option (b) is correct.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Students have asked these similar questions
Given: 2MNO(s) + O2(g) → 2MnO2(s) ArH = –269.6 kJ · mol-1
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced net equation for the reaction. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.) Help chemPad XXº → Greek How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCI? kJ How can you harness this reaction to do useful work? This is accomplished by making ---Select--- produce a voltage. cell that ---Select--- the reduction reaction and the oxidation reaction in order to control the flow of ---Select--- through a wire to
Consider the following reaction. (a) Is the reaction exothermic or endothermic? exothermic endothermic CH3OH(g) → CO(g) + 2 H₂(g) AH +90.7 kJ (b) Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. ΔΗ= 100.8 (c) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? 0.42 x g (d) How many kilojoules of heat are released when 13.0 g of CO(g) reacts completely with H₂(g) to form CH₂OH(g) at constant pressure? AH = -90.7 X kJ (e) Calculate AE when 400.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol K-41.7 XkJ HopHelpCh5N1

Chapter 8 Solutions

Student Solutions Manual for Ball's Physical Chemistry, 2nd

Ch. 8 - Prob. 8.11ECh. 8 - Prob. 8.12ECh. 8 - 8.13. Is the disproportionation reaction...Ch. 8 - Prob. 8.14ECh. 8 - Prob. 8.15ECh. 8 - Prob. 8.16ECh. 8 - Prob. 8.17ECh. 8 - 8.18. Determine and for each of the following...Ch. 8 - Prob. 8.19ECh. 8 - Prob. 8.20ECh. 8 - Prob. 8.21ECh. 8 - Prob. 8.22ECh. 8 - Prob. 8.23ECh. 8 - Prob. 8.24ECh. 8 - Prob. 8.25ECh. 8 - Prob. 8.26ECh. 8 - Prob. 8.27ECh. 8 - What is the Zn2+:Cu2+ ratio on a Daniell cell that...Ch. 8 - Prob. 8.29ECh. 8 - Determine the voltage of this reaction with the...Ch. 8 - The thermite reaction can act as the basis of an...Ch. 8 - A concentration cell has different concentrations...Ch. 8 - Prob. 8.34ECh. 8 - Prob. 8.35ECh. 8 - a What is the equilibrium constant for the...Ch. 8 - Prob. 8.37ECh. 8 - Prob. 8.38ECh. 8 - Prob. 8.39ECh. 8 - Prob. 8.40ECh. 8 - Prob. 8.41ECh. 8 - Consider the following formation reaction for HI:...Ch. 8 - Prob. 8.43ECh. 8 - 8.44. Determine an expression for , the change in...Ch. 8 - Prob. 8.45ECh. 8 - Prob. 8.46ECh. 8 - Determine the equilibrium constant for the...Ch. 8 - Prob. 8.48ECh. 8 - Prob. 8.49ECh. 8 - What is the solubility product constant of Hg2Cl2,...Ch. 8 - Prob. 8.51ECh. 8 - Prob. 8.52ECh. 8 - Prob. 8.53ECh. 8 - Prob. 8.54ECh. 8 - Prob. 8.55ECh. 8 - Prob. 8.56ECh. 8 - Prob. 8.57ECh. 8 - Show that a can be written as n+mnn+n+nn, where m...Ch. 8 - Prob. 8.59ECh. 8 - Prob. 8.60ECh. 8 - What molality of NaCl is necessary to have the...Ch. 8 - Prob. 8.62ECh. 8 - Prob. 8.63ECh. 8 - Calculate the molar enthalpy of formation of I(aq)...Ch. 8 - Prob. 8.65ECh. 8 - Hydrofluoric acid, HF(aq), is a weak acid that is...Ch. 8 - Prob. 8.68ECh. 8 - Prob. 8.69ECh. 8 - Prob. 8.70ECh. 8 - Prob. 8.71ECh. 8 - Prob. 8.72ECh. 8 - The mean activity coefficient for an aqueous...Ch. 8 - Human blood plasma is approximately 0.9NaCl. What...Ch. 8 - Under what conditions does the extended...Ch. 8 - Prob. 8.76ECh. 8 - Approximate the expected voltage for the following...Ch. 8 - Prob. 8.78ECh. 8 - Prob. 8.79ECh. 8 - Prob. 8.80ECh. 8 - a The salt NaNO3 can be thought of as...Ch. 8 - Prob. 8.82ECh. 8 - What is the estimated velocity for Cu2+ ions...Ch. 8 - Prob. 8.84ECh. 8 - Prob. 8.85ECh. 8 - Prob. 8.86ECh. 8 - Calculate a the solubility product constant for...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Text book image
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Text book image
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Text book image
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Electrolysis; Author: Tyler DeWitt;https://www.youtube.com/watch?v=dRtSjJCKkIo;License: Standard YouTube License, CC-BY