$CuSO_4$ solution is electrolysed for $15 \ minutes$ to deposit $0.4725 \ g$ of copper at the cathode. The current in amperes required is (Faraday $= 96,500 \ C \ mol^{-1}$,atomic weight of copper $= 63$)

An acidic solution of dichromate is electrolyzed for $8 \ min$ using $2 \ A$ current. As per the following equation: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. The amount of $Cr^{3+}$ obtained was $0.104 \ g$. The efficiency of the process (in $\%$) is (Take: $F = 96000 \ C$,At. mass of chromium $= 52$)

In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives

When $1 \ C$ of electricity is passed through an electrolytic solution,the mass deposited on the electrode is equal to which of the following?

$A$ current of $16\, A$ flows through molten $NaCl$ for $10\, min$. The amount of metallic sodium that appears at the negative electrode would be ............ $g$.

The cost of energy required to deposit $1 \ g$ of $Mg$ is $5.00$ rupees. What is the cost to deposit $10 \ g$ of $Al$? (Atomic mass of $Al = 27, Mg = 24$)