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(D) According to Faraday's second law of electrolysis,when the same quantity of electricity is passed through cells connected in series,the mass of th

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$3 : 2$

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(D) According to Faraday's second law of electrolysis,when the same quantity of electricity is passed through cells connected in series,the mass of the substance deposited is proportional to its equivalent weight $(E)$.The ratio of the mass of iron deposited is given by: $\frac{W_1}{W_2} = \frac{E_1}{E_2}$.For $FeCl_2$,the oxidation state of $Fe$ is $+2$,so the equivalent weight $E_1 = \frac{	ext{Atomic mass}}{2} = \frac{56}{2} = 28$.For $FeCl_3$,the oxidation state of $Fe$ is $+3$,so the equivalent weight $E_2 = \frac{	ext{Atomic mass}}{3} = \frac{56}{3} = 18.67$.Therefore,the ratio $\frac{W_1}{W_2} = \frac{56/2}{56/3} = \frac{3}{2} = 3:2$.

Two electrolytic cells,one containing acidified ferrous chloride $(FeCl_2)$ and the other containing acidic ferric chloride $(FeCl_3)$,are connected in series. When an electric current is passed through the cells,what is the ratio of iron deposited at the cathodes in the two cells?

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