What volume of chlorine gas (molar mass 71) is evolved at STP during electrolysis of fused NaCl by passage…

What volume of chlorine gas (molar mass 71) is evolved at STP during electrolysis of fused NaCl by passage of 1 amp current for 965 second? (At STP, V = $22.4 . \mathrm{dm}^3$ )
  1. 0.112 L
  2. $\quad 0.224 \mathrm{~L}$
  3. 1.12 L
  4. $\quad 2.24 \mathrm{~L}$

Solution

$2 \mathrm{Cl}^{-} \longrightarrow \mathrm{Cl}_2+2 \mathrm{e}^{-}$
For the reaction, mole ratio $=\frac{1}{2}$ Moles of product formed $\begin{aligned} & =\frac{\mathrm{I}(\mathrm{~A}) \times \mathrm{t}(\mathrm{~s})}{96500\left(\mathrm{C} \mathrm{~mol}^{-1}\right)} \times \text { mole ratio } \\ & =\frac{1 \times 965}{96500} \times \frac{1}{2} \\ & =5 \times 10^{-3} \mathrm{~mol} \end{aligned}$ $\begin{aligned} & \text { At STP, } 1 \mathrm{~mol} \mathrm{Cl}_{2(\mathrm{~g})}=22.4 \mathrm{dm}^3 \\ \therefore \quad & \text { At STP, } 5 \times 10^{-3} \mathrm{~mol} \mathrm{Cl}_{2(\mathrm{~g})}=0.112 \mathrm{~L} \end{aligned}$

Asked in: MHT CET 2024 (09 May Shift 1)

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