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Chemical Reactivity

The magnitude...

Question

The magnitude of standard Gibbs free energy for the given cell reaction in $K J m o l^{- 1} a t 298 K$ is
$Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q) + C u (s), E^{\circ} = 2 V a t 298 K$ $(F a r a d a y^{'} s c o n s t a n t, F = 96000 C m o l^{- 1})$

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Solution

Given $E^{\circ} = 2 V$
$Faraday's constant, F = 96000 C m o l^{- 1}$
$n = 2$
We know,
$Δ G^{\circ} = - n F E^{\circ} = - 2 \times 96000 \times 2 J / m o l$
$\Rightarrow Δ G^{\circ} = - 384000 J / m o l$
$\Rightarrow Δ G^{\circ} = - 384 K J / m o l$
So magnitude would be, $384 k J / m o l$

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