How much current is required to produce H_2 g | vedclass

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Question

(D) The reduction reaction for the production of $H_2$ gas is: $2H^{+} + 2e^{-} \longrightarrow H_2$. At $STP$,$1 \ mole$ of $H_2$ gas occupies $22400

Vedclass · Accepted Answer

$8.61$

Vedclass · Answer

(D) The reduction reaction for the production of $H_2$ gas is: $2H^{+} + 2e^{-} \longrightarrow H_2$. At $STP$,$1 \ mole$ of $H_2$ gas occupies $22400 \ cc$. From the reaction,$2 \ moles$ of electrons are required to produce $1 \ mole$ of $H_2$ gas. Charge required for $1 \ mole$ of $H_2 = 2 	imes 96500 \ C$. Therefore,charge required for $1 \ cc$ of $H_2 = \frac{2 	imes 96500}{22400} \approx 8.616 \ C$. Since the rate is $1 \ cc / sec$,the current $I = \frac{Q}{t} = \frac{8.616 \ C}{1 \ sec} = 8.616 \ A$. Thus,the required current is approximately $8.61 \ A$. Hence,option $(D)$ is correct.

How much current is required to produce $H_2$ gas at the rate of $1 \ cc / sec$ under $STP$ (in $A$)?

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