108 g silver (molar mass 108 g $m o l^{- 1}$ ) is deposited at cathode from $A g N O_{3} (a q)$ 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

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Solution

On applying Faraday's 1st law,
Moles of Ag deposited $= \frac{108}{108} = 1 m o l .$
$A g^{+} + e^{-} \to A g$
1 Faraday is required to deposit 1 mole of Ag.
$H_{2} O \to 2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-}$
$\frac{1}{2}$ Moles of $O_{2}$ are deposited by 2 F of charge.
This implies, 1 F will deposit $\frac{1}{4}$ moles of $O_{2}$
Using PV = nRT
P = 1bar
T = 273 K
R = 0.0823 L bar $m o l^{- 1} K^{- 1}$
On solving we get,
V = 5.68 L

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108 g silver (molar mass 108 g mol−1) is deposited at cathode from AgNO3(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

108 g silver (molar mass 108 g $m o l^{- 1}$ ) is deposited at cathode from $A g N O_{3} (a q)$ 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