The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

The electric charge for electrode deposition of one equivalent of a substance is equal to

The amount of $Ag$ (atomic mass $= 108$) deposited at the cathode when a current of $0.5 \, A$ is passed through a solution of $AgNO_3$ for $1 \, h$ is closest to $... \, g$.

When $10 \,A$ current is passed for $80 \,min$, the volume of hydrogen gas liberated at $STP$ is: (in $\,L$)

When a current of $10 \ A$ is passed through molten $AlCl_{3}$ for $1.608 \ minutes$,the mass of $Al$ deposited will be [Atomic mass of $Al = 27 \ g/mol$]:- (in $g$)

How many seconds of current at $9.65 \ A$ must be passed through a solution of $Al^{3+}$ to obtain $1 \ \text{millimole}$ of $Al$ metal?