A galvanic cell is constructed in which the overall reac-tion isPb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e)(a) Calculate AE° for this cell.(b) Chloride ions are added until PbCl, precipitates at theanode and [CI-] reaches 0.15 M. The cell potential isthen measured to be 0.22 V at pH = 0 and PH,1.0 atm. Calculate [Pb2+] under these conditions.(c) Calculate the solubility product constant Kp of PbCl2.

Given data are cell potential = 0.22V Cl- = 0.15M P H2 = 1.0 Atm. Pb2+ = ? ∆E = ? solubility…

A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O*(aq) → Pb²+ (aq) + H2 (g) + 2 H2O(€) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [Cl-1 reaches 0.15 M. The cell potential is

A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O*(aq) → Pb²+ (aq) + H2 (g) + 2 H2O(€) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [Cl-1 reaches 0.15 M. The cell potential is

Chemistry

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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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

A galvanic cell is constructed in which the overall reac-
tion is
Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e)
(a) Calculate AE° for this cell.
(b) Chloride ions are added until PbCl, precipitates at the
anode and [CI-] reaches 0.15 M. The cell potential is
then measured to be 0.22 V at pH = 0 and PH,
1.0 atm. Calculate [Pb2+] under these conditions.
(c) Calculate the solubility product constant Kp of PbCl2.

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