Choose the INCORRECT statement.A) The maximum work available in a cell = -zFEcell-B) AG° = -zFE°cellC) When Ecell < 0, the reaction is spontaneous.D) E°cell = 0 (zero) for a valid concentration cell.E) Reversing a cell reaction changes the sign of Ecell-Select one:а. АO b. BOc.O d. De.E

A Galvanic cell is an electrochemical cell, in which the chemical energy is converted into…

Choose the INCORRECT statement. A) The maximum work available in a cell = -zFEcell- B) AG° = -zFE°cell C) When Ecell < 0, the reaction is spontaneous. D) E°cel = 0 (zero) for a valid concentration cell. E) Reversing a cell reaction changes the sign of Ecell- Select one: Оа. А O b. B Ос. с O d. D Ое. Е

Choose the INCORRECT statement. A) The maximum work available in a cell = -zFEcell- B) AG° = -zFE°cell C) When Ecell < 0, the reaction is spontaneous. D) E°cel = 0 (zero) for a valid concentration cell. E) Reversing a cell reaction changes the sign of Ecell- Select one: Оа. А O b. B Ос. с O d. D Ое. Е

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 122AE: The overall reaction and equilibrium constant value for a hydrogen-oxygen fuel cell at 298 K is...

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If you calculate a value for G for a reaction using the values of Gf in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate G for a reaction at nonstandard conditions? The equation to determine G at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why dont reactions move away from equilibrium?
Calculate E°, G°, and K at 25°C for the reaction 3Mn2+(aq)+2MnO4(aq)+2H2O5MnO2(s)+4H+(aq)
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What is the maximum amount of electrical that is, non-pV work that can be obtained by reacting 1.00molCH4 in a fuel cell whose reaction is CH4(g)+2O2(g)2H2O(l)+CO2(g) at 25C?
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The table below lists relevant thermodynamic information for reactants and products in a hydrogen fuel cell. ΔfH° (kJ/mol) S° (J/mol·K) H2(g) 0 130.6 O2(g) 0 205.0 H2O(ℓ) -285.8 69.95 Compute ΔrG° at 25 °C and 70 °C (typical temperatures at which a hydrogen fuel cell operates).
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Consider the reaction AgCI (s) → Ag+ (aq) + Cl- (aq) (a) Calculate ΔG° at 25°C. (b) What should the concentration of Ag+ and CI- be so that ΔG = -1.0 kJ (just spontaneous)? Take [Ag+] = [Cl-]. (c) The Ksp for AgCl is 8 x 10-10. Is the answer to (b) reasonable?
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