To deposit one litre of hydrogen at 22.4 text | vedclass

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(D) The reaction for the liberation of hydrogen is: $2H^+ + 2e^- ightarrow H_2$.According to Faraday's law,$2 	ext{ moles}$ of electrons (i.e.,$2 \

Vedclass · Accepted Answer

$193000$

Vedclass · Answer

(D) The reaction for the liberation of hydrogen is: $2H^+ + 2e^- ightarrow H_2$.According to Faraday's law,$2 	ext{ moles}$ of electrons (i.e.,$2 	imes 96500 	ext{ C}$) are required to produce $1 	ext{ mole}$ of $H_2$ gas.At $NTP$ (or $STP$),$1 	ext{ mole}$ of any gas occupies $22.4 	ext{ L}$.Given that $22.4 	ext{ L}$ of $H_2$ is produced at $22.4 	ext{ atm}$ pressure,we use the ideal gas law $PV = nRT$ to find the moles of $H_2$.Since $P = 22.4 	ext{ atm}$,$V = 1 	ext{ L}$,$R = 0.0821 	ext{ L atm K}^{-1} 	ext{ mol}^{-1}$,the number of moles $n = \frac{PV}{RT}$.However,in standard electrolysis problems of this type,the question implies $1 	ext{ mole}$ of $H_2$ at $STP$ conditions ($1 	ext{ atm}$,$22.4 	ext{ L}$).If the question implies $1 	ext{ mole}$ of $H_2$ gas is produced,the charge required is $2 	imes 96500 	ext{ C} = 193000 	ext{ C}$.

To deposit one litre of hydrogen at $22.4 \text{ atmosphere}$ from acidulated water,the quantity of electricity that must pass through is ............. $coulomb$.

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