The potential of electrodes Cu2+ (aq) | Cu(s) is ϕ1 = 0.337 V , and Cu2+ (aq), Cu+ (aq) | Pt is ϕ2 = 0.153 V , respectively. a) Calculate the value of ϕ0 for electrode Cu+(aq) | Cu(s). [Hint: Write half reactions for the above two electrodes, then derive the target electrode.] b) Calculate the equilibrium constant Ka0 for the reaction Cu(s) + Cu2+ (aq) = 2Cu+ (aq) at 298.15K. [Hint: Based on the reaction, design a cell with two electrodes and verify that the two half reactions will give you the target reaction. Then calculate the cell potential.]
The potential of electrodes Cu2+ (aq) | Cu(s) is ϕ1 = 0.337 V , and Cu2+ (aq), Cu+ (aq) | Pt is ϕ2 = 0.153 V , respectively. a) Calculate the value of ϕ0 for electrode Cu+(aq) | Cu(s). [Hint: Write half reactions for the above two electrodes, then derive the target electrode.] b) Calculate the equilibrium constant Ka0 for the reaction Cu(s) + Cu2+ (aq) = 2Cu+ (aq) at 298.15K. [Hint: Based on the reaction, design a cell with two electrodes and verify that the two half reactions will give you the target reaction. Then calculate the cell potential.]
Chapter18: Introduction To Electrochemistry
Section: Chapter Questions
Problem 18.18QAP
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The potential of electrodes Cu2+ (aq) | Cu(s) is ϕ1 = 0.337 V , and Cu2+ (aq), Cu+ (aq) | Pt is ϕ2 = 0.153 V , respectively.
a) Calculate the value of ϕ0 for electrode Cu+(aq) | Cu(s). [Hint: Write half reactions for the above two electrodes, then derive the target electrode.]
b) Calculate the equilibrium constant Ka0 for the reaction Cu(s) + Cu2+ (aq) = 2Cu+ (aq) at 298.15K. [Hint: Based on the reaction, design a cell with two electrodes and verify that the two half reactions will give you the target reaction. Then calculate the cell potential.]
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