Question

An electric current of $1amp$ is passed through acidulated water for $160$ minutes and $50$ seconds. What is the volume of the hydrogen liberated at the anode (as reduced to NTP)?

• A. $1.12litre$
• B. $2.24litre$
• C. $11.2litre$
• D. $22.4litre$

Answer 1

The correct option is A $1.12litre$

Given Data : 1) Current =$I$= $1amp$

2) Time = $t$ = $160min50sec$ = $1950sec$

We know that,

$w$ = $\frac{M\times I\times t}{2\times 96500}$

But,

Number of moles = $n$ = $\frac{w}{M}$ = $\frac{I\times t}{2\times 96500}$

$n$ = $\frac{1\times 9650}{2\times 96500}$ = $0.05$ moles

1 mole of gas at NTP = $22.4l$

Hence volume of $0.05$ moles of hydrogen liberated = $22.4\times 0.05$ = $1.12l$

Hence the correct option is 'A'.