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

When same quantity of electricity is passed through $A g N O_{3}$ and $H_{2} S O_{4}$ solution connected in series 5.04 $\times 10^{- 2}$ g of $H_{2}$ is liberated. Calculate the mass of silver deposited:

Q. A constant electric current flows for

4

hours through two electrolytic cells connected in series. One contain

A g N O_{3}

solution and second contains

C u C l_{2}

solution. During this time,

4

grams of Ag are deposited in the first cell.
What is the current flowing in amperes?

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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 $\frac{n R T}{P} = \frac{0.25 \times 0.0821 \times 298}{\frac{750}{760}} = 6.2 L$ .