During the electrolysis of cupric chloride, the reactions occurring at electrodes are

At the anode:
$C u^{2 +} + 2 e^{-} \to C u (s)$

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At the cathode:
$2 C l^{-} \to C l_{2} (g) + 2 e^{-}$

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At the cathode:
$C u^{2 +} + 2 e^{-} \to C u (s)$

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At the anode:
$2 C l^{-} \to C l_{2} (g) + 2 e^{-}$

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Solution

The correct options are
C
At the cathode:
$C u^{2 +} + 2 e^{-} \to C u (s)$

D
At the anode:
$2 C l^{-} \to C l_{2} (g) + 2 e^{-}$

A little of cupric chloride is taken in a beaker. In the same beaker, two graphite rods are dipped and connected to 4.5 V battery. When electricity is passed through $C u C l_{2}$ solution, $C u$ and $C l_{2}$ are obtained.

Overall reaction: $C u C l_{2} (a q) \to C u (s) + C l_{2} (g)$

Reduction at the cathode: $C u^{2 +} + 2 e^{-} \to C u (s)$

Oxidation at the anode: $2 C l^{-} \to C l_{2} (g) + 2 e^{-}$

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Similar questions

Identify the correct reaction from the options given below for the electrolysis of $C u C l_{2}$ .

C u C l_{2}

Given are the reactions occuring during the electrolysis of sodium chloride solution:

$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?

E_{R P}

2 C l^{-} (a q .) \to C l_{2} (g) + 2 e^{-}

$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?

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