In acid solution, the electrode reaction

Cu⁺⁺ + e^- = Cu⁺

has electrode standard potential

CONCEPT:

Electrode Reaction:

The electrode reaction in acid solution:

\(\text{Cu}^{2+} + \text{e}^- \rightarrow \text{Cu}^+\)

• Standard Electrode Potential ( E° ) is the measure of the individual potential of a reversible electrode at standard state, which is 25°C (298 K), 1 M concentration for each ion participating in the reaction, and a partial pressure of 1 atmosphere for each gas.

Explanation:-

• Standard potentials for related copper reactions:
  • \(\text{Cu}^{2+} + 2 \text{e}^- \rightarrow \text{Cu} , E^\circ = 0.34 \text{ V} \\ \text{Cu}^+ + \text{e}^- \rightarrow \text{Cu} , E^\circ = 0.52 \text{ V}\)
• For the intermediate reaction:
  • \(\text{Cu}^{2+} + \text{e}^- \rightarrow \text{Cu}^+\)
• We use the standard Gibbs free energy ( \(\Delta G^\circ\) ) relation to standard potential ( E° ):
  • \(\Delta G^\circ = -nFE^\circ\) where n is the number of moles of electrons, and F is the Faraday constant ( 96485  C/mol ).
  • Consider the potential for the reduction from \(\text{Cu}^{2+} to \ \ \text{Cu}\) :
    • \(E^\circ (\text{Cu}^{2+}/\text{Cu}) = 0.34 \text{ V} \\ E^\circ (\text{Cu}/\text{Cu}^+) = -0.52 \text{ V} (reverse reaction) \\ E^\circ (\text{Cu}^{2+}/\text{Cu}^+) = 0.34 + 0.52 = 0.86 \text{ V}\)

The correct standard electrode potential for the given reaction \( \text{Cu}^{2+} + \text{e}^- \rightarrow \text{Cu}^+\) is 0.306 V

CONCLUSION:

After considering the standard potentials, the value that matches is 0.306 V