How many grams of chlorine gas will be produced as a product when a current of $2 \ A$ is passed through a concentrated aqueous solution of $NaCl$ for $30 \ \text{minutes}$?

In the electrolysis of an aqueous $Ni(NO_3)_2$ solution using $Ni$ electrodes,upon passing $1$ equivalent of charge,the mass of the cathode $(Ni = 59)$ changes by:

Calculate the mass of a divalent metal produced at the cathode by passing $5 \ A$ current through its salt solution for $100 \ minutes$. (Molar mass of metal $= x \ g/mol$)

Assertion $(A)$: The charge on one mole of electrons is one Faraday.
Reason $(R)$: The quantity of current required to deposit one mole of $Mg$ from $Mg^{2+}$ electrolyte solution is two Faradays.
The correct answer is

The weight of silver $(at. \ wt. = 108)$ displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $STP$ will be ............ $g.$

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