Laws of Electrolysis — MCQ Practice

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

Two electrolytic cells, one containing $AgNO_3$ solution and the other $CuSO_4$ solution, are connected in series. A current is passed until $1.08\,\text{g}$ of silver is deposited. What mass of copper will be deposited? (Given: Atomic mass of $Ag = 108\,\text{g/mol}$, $Cu = 63.5\,\text{g/mol}$)

Which of the following statements is INCORRECT regarding Faraday's First Law of Electrolysis?

How many Faradays of electricity are required to deposit $27\,\text{g}$ of aluminum from $Al_2O_3$ solution? (Given: Atomic mass of $Al = 27\,\text{g/mol}$)

A current of $2\,\text{A}$ is passed through an electrolytic cell containing $NiSO_4$ solution for $30\,\text{minutes}$. If the electrochemical equivalent of nickel is $0.000304\,\text{g/C}$, what mass of nickel will be deposited?

If $96500\,\text{C}$ of electricity is passed through a solution of $AlCl_3$, what volume of chlorine gas (at STP) would be liberated at the anode? (Given: Molar volume of gas at STP = $22.4\,\text{L/mol}$)