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Arrhenius Equation

The emf of th...

Question

The emf of the cell reaction,
$Z n (s) + {C u}^{2 +} (a q .) \to {Z n}^{2 +} (a q .) + C u (s)$
is $1.1 V$ . If enthalpy of the reaction is $- 216.7 k J {m o l}^{- 1}$ , calculate the entropy change for the reaction(in J/Kmole)

- 14.76

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- 29.5

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14.76

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29.5

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Solution

The correct option is A $- 14.76$
$- Δ G^{o} = n \times F \times E^{o} = 2 \times 96500 \times 1.1 = 212.3 k J$
$Δ G^{o} = - 212.3 k J {m o l}^{- 1}$
$Δ G^{o} = Δ H^{o} - T Δ S^{o}$
$Δ S^{o} = \frac{Δ H^{o} - Δ G^{o}}{T}$
$= \frac{- 216.7 - (- 212.3)}{298}$
$= - 0.01476 k J K^{- 1} {m o l}^{- 1}$
$= - 1476 J K^{- 1} {m o l}^{- 1}$

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