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Aqueous CuSO₄ is subjected to electrolysis using copper electrodes. If 6.36 grams of copper is deposited at cathode then (Aw of copper = 63.6)

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0.1 gram equivalents of copper decomposes at anode

0.05 gram equivalents of oxygen is liberated at anode

0.1 moles of copper decomposes at anode

0.56 litres of O₂ (at STP) is liberated at anode

answer is C.

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Detailed Solution

Cathode : ${Cu}^{2 +} = 2 e^{-} \to Cu (6.36 g)$
Anode : $\underset{(6.36 g)}{Cu} \to {Cu}^{2 +} + 2 e^{-}$
63.6 grams of ‘Cu’ = 1 mole = 2 gram equivalents
6.36 grams of ‘Cu’ = 0.1 moles = 0.2 gram equivalents

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