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(C) The electrode reaction for the liberation of hydrogen is: $2 H^+ + 2 e^- ightarrow H_2$.According to the reaction,$2 \, 	ext{moles}$ of electro

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$965 \, Coulomb$

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(C) The electrode reaction for the liberation of hydrogen is: $2 H^+ + 2 e^- ightarrow H_2$.According to the reaction,$2 \, 	ext{moles}$ of electrons (or $2 \, F$ of charge) are required to liberate $1 \, 	ext{mole}$ of $H_2$ gas.$1 \, 	ext{mole}$ of $H_2$ gas at $STP$ occupies $22400 \, cm^3$.Thus,$22400 \, cm^3$ of $H_2$ requires $2 \, F$ of electricity.Therefore,$112 \, cm^3$ of $H_2$ requires: $\frac{2 \, F 	imes 112 \, cm^3}{22400 \, cm^3} = 0.01 \, F$.Since $1 \, F = 96500 \, C$,the charge is $0.01 	imes 96500 \, C = 965 \, C$.

The quantity of electricity required to liberate $112 \, cm^3$ of hydrogen at $STP$ from acidified water is

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