What is the number of moles of electrons passed when a current of $2 \text{ A}$ flows through an electrolyte solution for $10 \text{ minutes}$?

The mass deposited at an electrode during electrolysis is directly proportional to which of the following?

When the same quantity of electricity is passed through aqueous $AgNO_3$ and $H_2SO_4$ solutions connected in series,$5.04 \times 10^{-2} \ g$ of $H_2$ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen $= 1.008$,silver $= 108$)

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

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

On passing a current through molten $KCl$,$19.5 \ g$ of potassium is deposited. If the same quantity of electricity is passed through molten aluminium chloride,then the amount of aluminium deposited will be ............. $g$.