The mass of silver (Molar mass of Ag: 108 g ) displaced by a quantity of electricity which displaces 5600 mL of ? at S.T.P. will be ______ g

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Solution

Q.
The mass of silver (Molar mass of Ag: 108 g ${mol}^{- 1}$ ) displaced by a quantity of electricity which displaces 5600 mL of $O_{2}$ at S.T.P. will be ______ g. [2024]

Ans.
(108)

Number of moles of oxygen at STP

$(n_{O_{2}}) = \frac{Volume at STP in mL}{22400} = \frac{5600}{22400} = 0.25 mol$

Oxidation of water to oxygen is represented as:

$2 H_{2} O \to O_{2} + 4 H^{+} + 4 e^{-}$

By stoichiometry: $\frac{n_{e^{-}}}{4} = \frac{n_{O_{2}}}{1}, \frac{n_{e^{-}}}{4} = \frac{0.25}{1}, n_{e^{-}} = 1 mol$

Reduction of silver to deposit silver metal is represented as:

${Ag}^{+} + e^{-} \to Ag$

By stoichiometry: $\frac{n_{Ag}}{1} = \frac{n_{e^{-}}}{1}, n_{Ag} = 1 mol$

Mass of silver deposited $= n_{Ag} \times M_{Ag} = 1 mol \times 108 {g mol}^{- 1} = 108 g$

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