Electrolysis — MCQ Practice

A current of $0.5,\text{A}$ is passed through a solution of $CuSO_4$ for $1,\text{hour}$. Calculate the mass of copper deposited at the cathode. (Given: Molar mass of $Cu = 63.5,\text{g/mol}$, $F = 96500,\text{C/mol}$)

During the electrolysis of a concentrated aqueous solution of $NaCl$ using inert electrodes, what are the products obtained at the anode and cathode, respectively?

Three electrolytic cells containing solutions of $AgNO_3$, $CuSO_4$, and $AlCl_3$ respectively, are connected in series. A steady current is passed through them until $1.08,\text{g}$ of silver is deposited. What mass of copper and aluminium will be deposited?

Which of the following statements about electrolysis is INCORRECT?

How many Faradays of electricity are required to deposit $2.7,\text{g}$ of aluminium from molten $Al_2O_3$?

During the electrolysis of aqueous $H_2SO_4$ using platinum electrodes, what is the gas liberated at the anode?