The amount of silver deposited on passing $2 \ F$ of electricity through an aqueous solution of $AgNO_3$ is: (in $g$)

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$

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:

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

The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?

Faraday's $2^{nd}$ law of electrolysis states that the mass of a substance deposited at an electrode is directly proportional to its: