Which of the following reaction correctly represents the oxidation process of Galvanic cell?

$C u (s) \to C u^{2 +} (a q) + 2 e^{-}$

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$Z n^{2 +} (a q) + 2 e^{-} \to Z n$

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$Z n (s) \to Z n^{2 +} (a q) + 2 e^{-}$

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$C u^{2 +} (a q) + 2 e^{-} \to C u$

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Solution

The correct option is C
$Z n (s) \to Z n^{2 +} (a q) + 2 e^{-}$

The device used for the conversion of chemical energy into electrical energy by redox process is called Galvanic cell. The redox process which occurs in Galvanic cell is:

At cathode: $C u^{2 +} (a q) + 2 e^{-} \to C u$ (Reduction)

At anode: $Z n (s) \to Z n^{2 +} (a q) + 2 e^{-}$ (Oxidation)

Suggest Corrections

Similar questions

The oxidation and reduction half reactions of the reaction

2Al_(s) + 3Cu²⁺_(aq) → 2Al³⁺_(aq) + 3Cu_(s) are

Z n^{2 +} (a q) + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{0} = 0.34 V

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

P b^{2 +} (a q) + 2 e^{-} \to P b (s); E^{0} = - 0.13 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

C u S O_{4}

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | | C u

0.350

C u^{2 +} (a q) + 2 e^{-} \to C u

- 0.763

Z n^{2 +} (a q) + 2 e^{-} \to Z n

C u_{(s)} \to C u_{(a q)}^{2 +} + 2 e^{-}; E^{o} = - 0.325 V

C u_{(a q)}^{+} + e^{-} \to C u_{(s)}; E^{o} = 0.50 V

E^{o}

2 C u_{(a q)}^{+} \to C u_{(a q)}^{2 +} + C u_{(s)}

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