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Electrolysis and Electrolytes

During anothe...

Question

During another seven minutes of electrolysis of aqueous copper sulphate solution after complete reduction of Cu ion, the substances evolved at cathode and anode are respectively:

Cu and O

_{2}

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_{2}

and O

_{2}

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Cu and H

_{2}

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Only O

_{2}

is evolved at cathode

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Solution

The correct option is B H $_{2}$ and O $_{2}$
The discharge potential of ${C u}^{2 +}$ ions is lower than $H^{+}$ ions. Hence ${C u}^{2 +}$ ions will be liberated at cathode in preference to $H^{+}$ ions. When during first seven minutes, all the copper is liberated at cathode, the hydrogen will start liberating.
The discharge potential of ${O H}^{-}$ ions is lower than ${S O}_{4}^{2 -}$ ions. Hence ${O H}^{-}$ ions will be liberated at anode (in the form of $O_{2}$ molecule) in preference to ${S O}_{4}^{2 -}$ ions.

Option B is correct.

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Similar questions

In the beginning of the electrolysis of aqueous copper sulphate solution, the substances evolved at cathode and anode are resepectively :

C u S O_{4}

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

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

[C u^{2 +}, O H^{-}, S O_{4}^{2 -}, H^{+}]

Aqueous $C u S O_{4}$ is electrolyzed using $A g$ as anode and $C u$ as cathode, then product of electrolysis at anode and cathode are, respectively

H_{2}

O_{2}

H_{2}

O_{2}

67.2 litres

H_{2}

S T P

C u

C u (I I)

C u

H_{2} + 2 O H^{-} \to 2 H_{2} O + 2 e^{-}

O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}

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