$Δ G^{o}$ of the cell reaction $A g C l (s) + 1 / 2 H_{2} (g) \to A g (s) + H^{+} (a q .) + {C l}^{-} (a q)$ is $- 21.52 k J$ .

Calculate the EMF for the cell reaction:
$2 A g C l (c) + H_{2} (g) \to A g (s) + 2 H^{+} (a q .) + 2 {C l}^{-} (a q .)$

0.223 V

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0.446 V

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0.112 V

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0.337 V

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Solution

The correct option is A $0.223 V$
We know, $Δ G = - n F E^{0}$

For the reaction, $A g C l (s) + 1 / 2 H_{2} (g) \to A g (s) + H^{+} (a q .) + {C l}^{-} (a q)$

$n = 1$

$- 21.52 \times 10^{3} = - 1 \times 96500 \times E^{0}$

$E^{0} = 0.223 V$

For reaction with $2 e^{-}$ transfer (2nd one) the E.M.F remains the same
$E^{0} = 0.223 V$

Suggest Corrections

Similar questions

Δ G^{o}

A g C l (s) + 1 / 2 H_{2} (g) ⟶ A g (s) + H^{+} + C l^{-}

- 21.52 k J

Δ G^{o}

2 A g C l (s) + H_{2} (g) \to 2 A g (s) + 2 H^{+} + 2 C l^{-}

1 / 2 H_{2} (g) + A g C l (s) \to H^{⨁} (a q) + C l^{⊝} (a q) + A g (s)

\frac{1}{2} H_{2} (g) + A g C l (s)

\to

H^{+} (a q .) + C l^{-} (a q .) + A g (s)

(1 / 2) H_{2} (g) + A g C l (s) = H^{+} (a q) + C l^{-} (a q) + A g (s)

\frac{1}{2} H_{2} (g) + A g C l (s) ⇌ H^{\oplus} (a q) + C l^{⊖} (a q) + A g (s)

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