When an electric current is passed through acidified water at $STP$,$112 \ mL$ of hydrogen gas is collected at the cathode in $965 \ s$. What is the current in amperes?

Salts of $A, B$ and $C$ were electrolysed under identical conditions using the same quantity of electricity. It was found that when $2.1 \ g$ of $A$ was deposited,the weights of $B$ and $C$ deposited were $2.7 \ g$ and $9.6 \ g$. If the atomic mass of $A, B$ and $C$ are $7, 27$ and $64$ respectively,then the valencies of $A, B$ and $C$ respectively are:

$A$ current of $2.0 \ A$ is passed for $5 \ hours$ through a molten metal salt,which deposits $22.2 \ g$ of metal (At. wt. $= 177$). The oxidation state of the metal in the metal salt is:

$A$ solution of a salt of a metal was electrolysed for $150$ minutes with a current of $0.15$ amperes. The weight of metal deposited was $0.783 \ g$. The equivalent weight of the metal is ................... $g$. (in $.97$)

To deposit one litre of hydrogen at $22.4 \text{ atmosphere}$ from acidulated water,the quantity of electricity that must pass through is ............. $coulomb$.

The value of current required to deposit $0.972 \ g$ of chromium in $3 \ hours$ if the $E.C.E.$ of chromium is $0.00018 \ g \ C^{-1}$,is ............ $A$.