First slide

Faraday's Laws

Question

A 4.0 M aqueous solution of NaCl is prepared and 500 mL of this solution is electrolyzed. This leads to evolution of chlorine gas at one of the electrodes.
(Q). The total charge required for the complete electrolysis will be

Moderate

A

96500 C
B

24125 C
C

48250 C
D

193000 C

Solution

$\begin{aligned} {Na}^{+} + e^{-} \overset{Hg}{⟶} Na (Hg) \\ 2 {Cl}^{-} ⟶ {Cl}_{2} + 2 e^{-} \end{aligned}$
Moles of NaCl electrolyzed is $4 \times \frac{500}{1000} = 2 .0$
Two Faraday of electric charge is required for electrolysis of 2 moles of NaCl.
Total coulombs = 2 x 96500= 193000 C.

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