$A$ 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:

$3.17 \ g$ of a substance is deposited by a current of $0.1 \ mol$ of electrons. What is the equivalent weight of the substance?

During electrolysis of an aqueous solution of $Na_{2}SO_{4}$,$2.4 \, L$ of $O_{2}$ at $STP$ was liberated at the anode. The volume of $H_{2}$ at $STP$ liberated at the cathode is ............. $L$.

An electric current is passed through silver nitrate solution using silver electrodes. $10.79 \ g$ of silver was found to be deposited on the cathode. If the same amount of electricity is passed through copper sulphate solution using copper electrodes,the weight of copper deposited on the cathode is ............. $g$

The unit of electrochemical equivalent is

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$