An electric current is passed through electrolytic cells in series one containing AgNO3 aq- and other H2SO4 aq- What volume of O2 in litre measured at 25-C and 750 mm Hg pressure would be liberated from H2SO4 ifone mole of Ag- is deposited from AgNO3 solution solution- write the value to the nearest integer

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Standard XII

Chemistry

Faraday's Second Law

An electric c...

Question

An electric current is passed through electrolytic cells in series one containing $A g (N O_{3})$ (aq.) and other $H_{2} S O_{4}$ (aq.). What volume of $O_{2}$ (in litre) measured at $25^{\circ} C$ and 750 mm Hg pressure would be liberated from $H_{2} S O_{4}$ ifone mole of $A g^{+}$ is deposited from $A g N O_{3}$ solution
solution. (write the value to the nearest integer)

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Solution

The deposition of one mole of Ag corresponds to 1 faraday of charge.
1 faraday of charge will liberate 0.25 moles of oxygen which corresponds to a volume of $\frac{n R T}{P} = \frac{0.25 \times 0.0821 \times 298}{\frac{750}{760}} = 6.2 L$ .

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The deposition of one mole of Ag corresponds to 1 faraday of charge.1 faraday of charge will liberate 0.25 moles of oxygen which corresponds to a volume of nRTP=0.25×0.0821×298750760=6.2L.

The deposition of one mole of Ag corresponds to 1 faraday of charge.
1 faraday of charge will liberate 0.25 moles of oxygen which corresponds to a volume of $\frac{n R T}{P} = \frac{0.25 \times 0.0821 \times 298}{\frac{750}{760}} = 6.2 L$ .