108 g of 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 ______ (up to two decimel)

5.67

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5.670

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Solution

Number of moles of $A g (s)$ gets deposited,
$n_{A g} = \frac{108}{108} = 1 m o l$

$A g^{+} + 1 e^{-} \to A g (s)$

$1 F$ charge is required for 1 mol of Ag

Electrolysis of water:
Oxidation reaction,
$H_{2} O \to \frac{1}{2} O_{2} + 2 H^{+} + 2 e^{-}$

$\frac{1}{2}$ $mole$ of $O_{2}$ liberated from 2 F charge.
Thus,
$\frac{1}{4}$ $mole$ of $O_{2}$ liberated from 1 F charge.

By gas law,
$P V = n R T$

$V = \frac{1}{4} \times \frac{0.083 \times 273}{1}$

$V = 5.675 L$

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108 g of 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 ______ (up to two decimel)

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