Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by $1 \ A$ 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.
(B) The mass of copper and silver deposited will be different.
According to Faraday's second law of electrolysis,the mass $(m)$ of a substance deposited is given by $m = \frac{M \times I \times t}{n \times F}$,where $M$ is the molar mass,$I$ is the current,$t$ is the time,$n$ is the number of electrons involved in the reduction,and $F$ is Faraday's constant.
For $Ag^+$: $Ag^+ + e^- \rightarrow Ag$,so $n = 1$.
For $Cu^{2+}$: $Cu^{2+} + 2e^- \rightarrow Cu$,so $n = 2$.
Since the equivalent weights $(M/n)$ of $Cu$ $(63.5/2 = 31.75 \ g/mol)$ and $Ag$ $(107.8/1 = 107.8 \ g/mol)$ are different,the masses deposited will be different even when the same quantity of electricity $(Q = I \times t)$ is passed.
According to Faraday's second law of electrolysis,the mass $(m)$ of a substance deposited is given by $m = \frac{M \times I \times t}{n \times F}$,where $M$ is the molar mass,$I$ is the current,$t$ is the time,$n$ is the number of electrons involved in the reduction,and $F$ is Faraday's constant.
For $Ag^+$: $Ag^+ + e^- \rightarrow Ag$,so $n = 1$.
For $Cu^{2+}$: $Cu^{2+} + 2e^- \rightarrow Cu$,so $n = 2$.
Since the equivalent weights $(M/n)$ of $Cu$ $(63.5/2 = 31.75 \ g/mol)$ and $Ag$ $(107.8/1 = 107.8 \ g/mol)$ are different,the masses deposited will be different even when the same quantity of electricity $(Q = I \times t)$ is passed.
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