Question

The electrode potentials for \[ \text{Cu}^{2+}(aq) + e^- \rightleftharpoons \text{Cu}(s) \] \text{and} \[ \text{Cu}^{2+}(aq) + e^- \rightleftharpoons \text{Cu}(aq) \] \text{are +0.15 V and +0.50 V, respectively. The value of \( E^\circ_{\text{Cu}^{2+}/\text{Cu}} \) will be:}

• A. 0.500 V
• B. 0.325 V
• C. 0.650 V
• D. 0.150 V

Hint:

The standard electrode potential for a half-reaction is determined from the potential difference between the cathode and anode.

Answer 1

The Correct Option is A

The standard electrode potential is calculated using the formula: \[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \] Using the given values for the electrode potentials and the relationship between the half-reactions, we calculate \( E^\circ_{\text{Cu}^{2+}/\text{Cu}} \) as 0.500 V.
Final Answer: \[ \boxed{0.500 \, \text{V}} \]