What is the quantity of electricity in Faradays required to produce $8 \text{ g}$ of $Mg$ (molar mass = $24 \text{ g mol}^{-1}$) from $MgCl_2$ solution (in $\text{ F}$)?

The electrochemical equivalent of a metal is $3.3 \times 10^{-7} \ kg/C$. The mass of the metal liberated at the cathode when a $3 \ A$ current is passed for $2 \ s$ will be:

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

$9.65 \ C$ of electric current is passed through fused anhydrous $MgCl_2$. The magnesium metal thus obtained is completely converted into a Grignard reagent. The number of moles of Grignard reagent obtained is

$A$ $200 \ W, 100 \ V$ bulb is connected in series with an electrolytic cell. If an aqueous solution of an $Sn$-salt is electrolysed for $5 \ hrs$,$11.1 \ g$ of $Sn$ gets deposited. The chemical formula of the compound is (Given atomic weight of $Sn$ is $118.7 \ g \ mol^{-1}$).

In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ \text{minutes}$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ \text{seconds}$ will be: