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Equilibrium Constant and Standard Free Energy Change

The standard ...

Question

The standard electrode potential of a Daniell cell is $1.1 V$ . Find the standard Gibbs energy for the reaction.
$Z n (s) + C u^{2 +} (a q .) \to Z n^{2 +} (a q .) + C u (s)$

- 212.3 kJ/mol

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- 2.123 kJ/mol

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- 21.23 kJ/mol

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- 21230 kJ/mol

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Solution

The correct option is A $- 212.3 kJ/mol$
For the reaction $n = 2$
$F = 96500 C/mol$ and $E = 1.1 V$
$∵ Δ_{r} G^{o} = - 2 \times 1.1 \times 96500 = - 212300 J/mol = - 212.3 kJ/mol$

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