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Representation of Cell

Zns | ZnCl2aq...

Question

$Z n (s) | Z n C l_{2} (a q) | | C l^{-} (a q) | C l_{2} (g) | C (s)$
In the electrochemical cell described by the cell diagram above, what reaction occurs at the anode?

Z n \to Z n^{2 +} + 2 e

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Z n^{2 +} + 2 e \to Z n

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C l_{2} + 2 e \to 2 C l^{-}

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2 C^{-} \to C l_{2} + 2 e

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Z n + C l_{2} \to Z n C l_{2}

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Solution

The correct option is B $Z n \to Z n^{2 +} + 2 e$
At anode oxidation will take place and the anode reaction can be written as:
Oxidation reaction: $Z n \to Z n^{2 +} + 2 e^{-}$

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Similar questions

Z n (s) | Z n {C l}_{2} (a q) | ∣ ∣ {C l}^{-} (a q) ∣ ∣ | {C l}_{2} (g) | C (s)

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

Z n \to Z n^{2 +} + 2 e^{-} (E_{(Z n^{2 +} / Z n)}^{0} = - 0.76 V)

F e \to F e^{2 +} + 2 e^{-} E^{0} = 0.41 V

F e^{2 +} + Z n \to Z n^{2 +} + F e

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

Z n ∣ ∣ {Z n}^{2 +} (a q) ∣ ∣ ∣ ∣ {C u}^{2 +} (a q) ∣ ∣ C u

{C u}^{2 +} + {2 e}^{-} ⟶ C u, E^{\circ} = + 0.35 V

{Z n}^{2 +} + {2 e}^{-} ⟶ Z n, E^{\circ} = - 0.763 V

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