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What amount of $\mathrm{Cl}_2$ gas liberated at anode, if 1 ampere current is passed for 30 minute from NaCl solution?
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The correct answer is:
0.66 g
$2 \mathrm{Cl}^{-} \rightarrow \underset{1 \text { mole }}{\mathrm{Cl}_2}+\underset{2 \times 96500 \text { coulomb }}{2 e^{-} \text {(At anode) }}$
$\begin{aligned} Q & =i t=1 \times 30 \times 60 \\ & =1800 \text { coulomb }\end{aligned}$
The amount of chlorine liberated by passing 1800 coulomb of electric charge
$=\frac{1 \times 1800 \times 71}{2 \times 96500}=0.66 \mathrm{~g}$
$\begin{aligned} Q & =i t=1 \times 30 \times 60 \\ & =1800 \text { coulomb }\end{aligned}$
The amount of chlorine liberated by passing 1800 coulomb of electric charge
$=\frac{1 \times 1800 \times 71}{2 \times 96500}=0.66 \mathrm{~g}$
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