The reaction,

$(1 / 2) H_{2} (g) + A g C l (s) = H^{+} (a q) + C l^{-} (a q) + A g (s)$ occurs in the galvanic cell

The correct cell representation is given by _____________.

A g | A g C l (s) | K C l (s o l n .) | A g N O_{3} (s o l n .) | A g

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P t | H_{2} (g) | H C l (s o l n .) | A g N O_{3} (s o l n .) | A g

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P t | H_{2} (g) | H C l (s o l n .) | A g C l (s) | A g (s)

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P t | H_{2} (g) | K C l (s o l n .) | A g C l (s) | A g

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Solution

The correct option is B $P t | H_{2} (g) | H C l (s o l n .) | A g C l (s) | A g (s)$
$\frac{1}{2} H_{2} ⟶ H^{+} + e^{-}$ (anode)

$A g C l + e^{-} ⟶ A g + {C l}^{-}$ (cathode)

So cell representation : $P t | H_{2} (g) | H C l ({s o l}^{n}) | A g C l (s) | A g (s)$

Suggest Corrections

Similar questions

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)

Δ G^{o}

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

- 21.52 k J

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

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

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

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