A solution of copper sulphate is electrolyzed for 10 minutes with a current of 1.5 amperes. The mass

Question

A solution of copper sulphate is electrolyzed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at cathode is:

(Given: Molar mass of $Cu = 63\text{ }g{\text{ }mol}^{- 1}$;

$1\text{ }F = 96487C{mol}^{- 1}$ )

Accepted Answer

Sol. [Key Concept: Faraday's laws of electrolysis: m = (E·I·t)/F] ${CuSO}_{4} \longrightarrow {Cu}^{2 +} + {SO}_{4}^{2 -}$$$\begin{matrix} 2e^{-} & \ + {Cu}^{2 +} \longrightarrow Cu(	ext{ }s) \ W & \ = zit \ & \ = \frac{E 	imes it}{96500} \ & \ = \frac{63 	imes 1.5 	imes 10 	imes 60}{2 	imes 96500} \ & \ = \frac{56,700}{193000} = 0.2938	ext{ }g \end{matrix}$$

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