A copper concentration cell is composed of the following half-cells: the cathode half-cell contains a copper electrode in 1.0 M CuSO4 solution, while the anode half-cell contains a copper electrode in a solution that contains an equilibrium mixture of Cu2+, Cu(NH3)42+, and NH3. The concentrations of the complex-ion Cu(NH3)42+ and NH3 are 0.010 M and 3.0 M, respectively, but the equilibrium concentration of Cu2+(aq) is unknown and will be determined from the cell voltage. If the concentration cell shows an Ecell = 0.51 V, calculate the concentration of Cu2+ in the anode half-cell. (A) 4.2 x 108 M (B) 2.4 x 10–9 M (C) 5.8 x 10–18 M (D) 2.0 x 104 M
A copper concentration cell is composed of the following half-cells: the cathode half-cell contains a copper electrode in 1.0 M CuSO4 solution, while the anode half-cell contains a copper electrode in a solution that contains an equilibrium mixture of Cu2+, Cu(NH3)42+, and NH3. The concentrations of the complex-ion Cu(NH3)42+ and NH3 are 0.010 M and 3.0 M, respectively, but the equilibrium concentration of Cu2+(aq) is unknown and will be determined from the cell voltage. If the concentration cell shows an Ecell = 0.51 V, calculate the concentration of Cu2+ in the anode half-cell. (A) 4.2 x 108 M (B) 2.4 x 10–9 M (C) 5.8 x 10–18 M (D) 2.0 x 104 M
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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A copper concentration cell is composed of the following half-cells: the cathode half-cell contains a copper electrode in 1.0 M CuSO4 solution, while the anode half-cell contains a copper electrode in a solution that contains an equilibrium mixture of Cu2+, Cu(NH3)42+, and NH3. The concentrations of the complex-ion Cu(NH3)42+ and NH3 are 0.010 M and 3.0 M, respectively, but the equilibrium concentration of Cu2+(aq) is unknown and will be determined from the cell voltage. If the concentration cell shows an Ecell = 0.51 V, calculate the concentration of Cu2+ in the anode half-cell.
(A) 4.2 x 108 M
(B) 2.4 x 10–9 M
(C) 5.8 x 10–18 M
(D) 2.0 x 104 M
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