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(D) According to Faraday's laws of electrolysis,the amount of chemical change produced by an electric current is proportional to the quantity of elect

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$96500 \, 	ext{coulombs}$

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(D) According to Faraday's laws of electrolysis,the amount of chemical change produced by an electric current is proportional to the quantity of electricity passed through the electrolyte.One gram equivalent of any substance is deposited by the passage of $1 \, 	ext{Faraday}$ of electricity.$1 \, 	ext{Faraday} = 96500 \, 	ext{coulombs}$.Therefore,$96500 \, 	ext{coulombs}$ of charge is required to deposit one gram equivalent of an element at an electrode.

Column $I$ (Reduction process)	Column $II$ (Charge required)
$(a)$ $1$ mol of $MnO_4^-$ to $Mn^{2+}$	$(p)$ $193000$ $C$
$(b)$ $1$ mol of $Cr_2O_7^{2-}$ to $Cr^{3+}$	$(q)$ $289500$ $C$
$(c)$ $1$ mol of $Sn^{4+}$ to $Sn^{2+}$	$(r)$ $482500$ $C$
$(d)$ $1$ mol of $Al^{3+}$ to $Al$	$(s)$ $579000$ $C$

To deposit one $gm$ equivalent of an element at an electrode,the quantity of electricity needed is

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