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The dissolution reaction of a sparingly soluble PbSO4 salt is given by, => PbSO4 (s) ------> Pb2+ (aq) + SO42- (aq) b) The half reactions given are, 1) Pb2+ (aq) + 2 e- -------> Pb (s)                          Eored = -0.1262 V 2) PbSO4 (s) + 2 e- -----> Pb (s) + SO42- (aq)         Eored = -0.3505 V => Pb2+ (aq) + SO42- (aq) -------> PbSO4 (s)                   E = -0.1262 - (-0.3505) = 0.2243 V Hence the cell potential is 0.2243 V.

The dissolution reaction of a sparingly soluble PbSO4 salt is given by, => PbSO4 (s) ------> Pb2+ (aq) + SO42- (aq) b) The half reactions given are, 1) Pb2+ (aq) + 2 e- -------> Pb (s)                          Eored = -0.1262 V 2) PbSO4 (s) + 2 e- -----> Pb (s) + SO42- (aq)         Eored = -0.3505 V => Pb2+ (aq) + SO42- (aq) -------> PbSO4 (s)                   E = -0.1262 - (-0.3505) = 0.2243 V Hence the cell potential is 0.2243 V.

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The dissolution reaction of a sparingly soluble PbSO4 salt is given by,

=> PbSO4 (s) ------> Pb2+ (aq) + SO42- (aq)

b) The half reactions given are,

1) Pb2+ (aq) + 2 e- -------> Pb (s)                          Eored = -0.1262 V

2) PbSO4 (s) + 2 e- -----> Pb (s) + SO42- (aq)         Eored = -0.3505 V

=> Pb2+ (aq) + SO42- (aq) -------> PbSO4 (s)                   E = -0.1262 - (-0.3505) = 0.2243 V

Hence the cell potential is 0.2243 V.

E° red Pb²*(aq) + 2e- → Pb(s) 0.1262 V Ered PBSO«(s) + 2e- → Pb(s) + SO,²(aq) 0.3505 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b. d) Using only the information provided in this problem, calculate the solubility product constant of lead(II) sulfate at 10, °C. e) Is the dissolution of lead(11) sulfate at 10. °C thermodynamically favorable? Justify your response by determining AG°n at 10. °C, using only the information provided or determined in this problem.
Transcribed Image Text:E° red Pb²*(aq) + 2e- → Pb(s) 0.1262 V Ered PBSO«(s) + 2e- → Pb(s) + SO,²(aq) 0.3505 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b. d) Using only the information provided in this problem, calculate the solubility product constant of lead(II) sulfate at 10, °C. e) Is the dissolution of lead(11) sulfate at 10. °C thermodynamically favorable? Justify your response by determining AG°n at 10. °C, using only the information provided or determined in this problem.
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