How much current should be passed through aci | vedclass

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(B) The reaction for the liberation of $H_2$ is: $2H^+ + 2e^- \rightarrow H_2(g)$.$22.4 \ L$ of $H_2$ at $STP$ corresponds to $1 \ mole$ of $H_2$.To p

Vedclass · Accepted Answer

$19.3$

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(B) The reaction for the liberation of $H_2$ is: $2H^+ + 2e^- ightarrow H_2(g)$.$22.4 \ L$ of $H_2$ at $STP$ corresponds to $1 \ mole$ of $H_2$.To produce $1 \ mole$ of $H_2$,$2 \ moles$ of electrons are required,which is equal to $2 \ F$ of charge $(2 	imes 96500 \ C)$.Charge required to liberate $0.224 \ L$ of $H_2 = \frac{2 	imes 96500 \ C}{22.4 \ L} 	imes 0.224 \ L = 2 	imes 965 \ C = 1930 \ C$.Using the formula $Q = I 	imes t$,where $t = 100 \ s$:$I = \frac{Q}{t} = \frac{1930 \ C}{100 \ s} = 19.3 \ A$.

How much current should be passed through acidified water for $100 \ s$ to liberate $0.224 \ L$ of $H_2$ gas at $STP$ (in $A$)?

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