On passing $3 \ A$ of electricity for $50 \ minutes$,$1.8 \ g$ of metal deposits. The equivalent mass of the metal is:

In the electrolysis of acidulated water,it is desired to obtain $1.12 \ cc$ of hydrogen gas per second at $STP$ conditions. The current to be passed is: (in $A$)

$A$ constant current was passed through a solution of $AuCl_4^-$ ion between gold electrodes. After a period of $10.0 \ \text{minutes}$,the increase in mass of cathode was $1.314 \ \text{g}$. The total charge passed through the solution is . . . . . . $\times 10^{-2} \ \text{F}$. (Given atomic mass of $Au = 197$)

The number of electrons involved in redox reactions when $1$ Faraday of electricity is passed through an electrolyte in solution is

Same amount of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$. The number of $Ag$ and $Cu$ atoms deposited are $x$ and $y$ respectively. The correct relationship between $x$ and $y$ is

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).