Which of the following reaction taken place at anode during electroplating of metal with silver using sodium argentocyanide as an electrolyte?

A g - e^{_} ⟶ {A g}^{+}

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{A g}^{+} + e^{_} ⟶ A g

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A g - 2 e^{_} ⟶ {A g}^{+} + e^{-}

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2 {A g}^{+} + e^{_} ⟶ A g

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Solution

The correct option is A $A g - e^{_} ⟶ {A g}^{+}$
In electroplating with silver, oxidation reaction at anode takes place:

$A g - e^{-} \to A g^{+}$ .

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Similar questions

The standard oxidation potential of zinc and silver in water at 298 K are

Which of the following reactions actually take place

E^{\circ}

2 A g + Z n^{2 +} \to 2 A g^{+} + Z n

E_{A g^{+} / A g}^{\circ} = 0.80 V, E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V

E^{\circ}

298 K

A g (N H_{3})_{2}^{+} + e^{-} \to A g + 2 N H_{3}

A g^{+} + e^{-} \to A g; E_{A g^{+} / A g}^{\circ} = 0.80 V

A g (N H_{3})_{2}^{+} ⇌ A g^{+} + 2 N H_{3}; K = 6 \times 10^{- 8}

C u (s) | C u^{2 +} (a q) | | A g^{+} (a q) | A g (s)

Z n^{+ 2} + 2 e^{-} ⇌ Z n; E^{o} = - 0.76 V

A g^{+} + e^{-} ⇌ A g; E^{o} = + 0.80 V

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