Question

The standard potential of the cell in the following reaction is ______________.
Cd(s) + Cu\(^{2+}\) (aq) \to Cd\(^{2+}\) (aq) + Cu(s)
(E\(^\circ\)_Cd = -0.403 V, E\(^\circ\)_Cu = 0.334 V)

• A. -0.069 V
• B. 0.737 V
• C. -0.737 V
• D. 0.069 V

Answer 1

The Correct Option is B

Standard cell potential: \( E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \).
Cathode (reduction): Cu\(^{2+}\) + 2e\(^- \to \) Cu, \( E^\circ_{\text{Cu}} = 0.334 \, \text{V} \).
Anode (oxidation): Cd \to Cd\(^{2+}\) + 2e\(^-\), \( E^\circ_{\text{Cd}} = -0.403 \, \text{V} \).
\[ E^\circ_{\text{cell}} = 0.334 - (-0.403) = 0.334 + 0.403 = 0.737 \, \text{V}. \] Answer: 0.737 V.