$2.644 \ g$ of metal $(M)$ was deposited when $8040 \ C$ of electricity was passed through molten $MF_2$ salt. What is the atomic mass of $M$ $(F = 96500 \ C \ mol^{-1})$ (in $u$)?

When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their:

$A$ current of $10.0 \, A$ flows for $2.00 \, h$ through an electrolytic cell containing a molten salt of metal $X$. This results in the decomposition of $0.250 \, mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is $(F = 96,500 \, C \, mol^{-1})$ (in $+$)

The current flowing in a copper voltameter is $3.2 \ A$. The number of copper ions $(Cu^{2+})$ deposited at the cathode per minute is

In electrolysis,if the duration of the passage of current is doubled,the mass liberated is

How long should aqueous $NaCl$ be electrolysed by passing $100 \ A$ current,so that $0.5 \ mol$ chlorine is released at anode?