Given the standard potential for the following half-cell reaction at 298 K,

$C u^{+} (a q) + e^{-} \to C u (s);$ $E ° = 0.52$ V

$C u^{2 +} (a q) + e^{-} \to C u^{+} (a q);$ $E ° = 0.16$ V

Calculate the $Δ G °$ (kJ) for the reaction, $[2 C u^{+} (a q) \to C u (s) + C u^{2 +}]$

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TestHub · Accepted Answer

C u + + e - → C u ; E ° = 0.52 V Δ G 1 = - n F E ° = - 1 × 96500 × 0.52 ...(i) C u 2 + + e - → C u + ; E ° = 0.16 V or C u + → C u 2 + + e - ; E ° = - 0.16 V Δ G 2 = - 1 × 96500 × - 0.16 ...(ii) On adding equations (i) and (ii), we get 2 C u + → C u + C u 2 + , Δ G = Δ G 1 + Δ G 2 = - 96500 × 0.52 + 96500 × 0.16 = 96500 - 0.52 + 0.16 = - 96500 × 0.36 = − 34740 J = − 34 .740 kJ

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