$A$ solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at the cathode is:
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)

$Assertion (A)$: $A$ current of $96.5 \ A$ is passed into aqueous $AgNO_3$ solution for $100 \ s$. The weight of silver deposited is $10.8 \ g$ (At. wt. of $Ag = 108$).
$Reason (R)$: The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
The correct answer is :

The amount of metal deposited at the cathode on passing an electric current of $0.75 \ A$ in an aqueous ferric sulphate solution for $30 \ min$ will be - ........... $g$ (atomic weight of $Fe = 56$).

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

How many atoms of calcium will be deposited from a solution of $CaCl_2$ by a current of $0.25 \, mA$ flowing for $60 \, s$?

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to: