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Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.
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According to Faraday's second law of electrolysis when the same quantity of electricity is passed through different electrolytes, the amounts of different substances formed are proportional to their chemical equivalent.
$\frac{W_1}{W_2}=\frac{E_1}{E_2}$
Since $E_1$ and $E_2$ have different values for $\mathrm{Cu}$ and $\mathrm{Ag}$ respectively depending upon the number of electrons required to reduce the respective metal ion. Therefore masses of Cu and Ag deposited will be different.
$\frac{W_1}{W_2}=\frac{E_1}{E_2}$
Since $E_1$ and $E_2$ have different values for $\mathrm{Cu}$ and $\mathrm{Ag}$ respectively depending upon the number of electrons required to reduce the respective metal ion. Therefore masses of Cu and Ag deposited will be different.
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