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Application of Electrolysis

1 M aqueous s...

Question

$1 M$ aqueous solution of $N a C l$ undergoes electrolysis if $50 m A$ current is passed for $12 h o u r s$ and efficiency is $25$ %. The total volume of gas produced at standard state is:

137 m l

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68.5 m l

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125.44 m l

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62 m l

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Solution

The correct option is D $125.44 m l$
At anode, in $1 m o l e N a C l 71.0 g m C l^{-}$ ion is present.

$2 C l^{-} \to C l_{2} + 2 e^{-}$

$71.0 g$ $71.0 g$ $2 \times 96500 C$

Charge $= Q = i \times t \times e f f i c i e n c y = 50 \times 10^{- 3} \times 12 \times 3600 \times \frac{1}{4}$

Moles of $C l_{2}$ liberated $= \frac{1}{2 \times 96500 \times 50 \times 10^{- 3} \times 12 \times 3600 \times \frac{1}{4}} = 2.8 m i l i m o l e s$

At cathode:

$2 e^{-} + 2 H_{2} O \to H_{2} (g) + 2 O H^{-} (a q)$

Moles of $H_{2}$ liberated $=$ moles of $C l_{2}$ liberated $= 2.8 m i l i m o l e s$

Total moles $= 5.6 m i l i m o l e s (C l_{2} + H_{2})$

Total volume of gas liberated as STP $= \frac{5.6}{1000} \times 22.4 \times 1000 = 125.44 m l$

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1 M aqueous solution of NaCl undergoes electrolysis if 50 mA current is passed for 12 hours and efficiency is 25%. The total volume of gas produced at standard state is:

$1 M$ aqueous solution of $N a C l$ undergoes electrolysis if $50 m A$ current is passed for $12 h o u r s$ and efficiency is $25$ %. The total volume of gas produced at standard state is: