Question

For the following cell, standard potential of copper electrode is 0.337 V and standard cell potential is 0.463 V.
Cu\(^{2+}\) (1M) / Cu (1M) || Ag\(^+\) (1M) / Ag What is the standard potential of silver electrode?

• A. -0.126 V
• B. 0.800 V
• C. -0.463 V
• D. 0.126 V

Hint:

To calculate the electrode potential in electrochemical cells, use the Nernst equation and account for the standard electrode potentials of each half-reaction.

Answer 1

The Correct Option is B

Step 1: Applying the Nernst equation.
We can use the Nernst equation to solve for the potential of the silver electrode. The standard cell potential is related to the potentials of the half-reactions by: \[ E_{\text{cell}} = E_{\text{cathode}} - E_{\text{anode}} \] Here, Cu\(^{2+}\) / Cu is the anode and Ag\(^+\) / Ag is the cathode. Thus, \[ 0.463 = E_{\text{Ag}} - 0.337 \quad \Rightarrow \quad E_{\text{Ag}} = 0.800 \, \text{V} \]
Step 2: Conclusion.
The standard potential of the silver electrode is (B) 0.800 V.