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(B) According to Faraday's law of electrolysis,the number of gram equivalents of substances deposited or liberated at electrodes is equal for the same

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$5.67$

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(B) According to Faraday's law of electrolysis,the number of gram equivalents of substances deposited or liberated at electrodes is equal for the same quantity of electricity passed.$1.$ Number of gram equivalents of $Ag = \frac{	ext{mass}}{	ext{equivalent mass}} = \frac{108 \ g}{108 \ g \ mol^{-1}} = 1 \ eq$.$2.$ Therefore,gram equivalents of $O_2(g)$ produced = $1 \ eq$.$3.$ The reaction for the evolution of $O_2$ from water is: $2H_2O ightarrow O_2 + 4H^+ + 4e^-$. The n-factor for $O_2$ is $4$.$4.$ Moles of $O_2 = \frac{	ext{gram equivalents}}{	ext{n-factor}} = \frac{1}{4} = 0.25 \ mol$.$5.$ At $273 \ K$ and $1 \ bar$ pressure $(STP)$,the molar volume of an ideal gas is $22.7 \ L \ mol^{-1}$.$6.$ Volume of $O_2 = 0.25 \ mol 	imes 22.7 \ L \ mol^{-1} = 5.675 \ L$.

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

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