Calculate moles of electrons, current, time, mass of substance or volume of gas produced or used during electrolysis. (Formula: q = 𝑛(e−) × F or q = I × t).

During the electrolysis of molten sodium chloride, a constant current of 4.85 A is passed through the cell for 1,930 seconds. Calculate the number of moles of electrons transferred during this electrolysis. (Faraday's constant = 96,485 C mol$^{-1}$)

During the electrolysis of copper(II) sulphate solution, copper metal is deposited on the cathode according to the equation $\text{Cu}^{2+}(\text{aq}) + 2e^- \to \text{Cu}(\text{s})$. A constant current of 2.5 A is passed through the electrolytic cell for 1,930 seconds. Calculate the mass of copper deposited on the cathode. Show your working.

During the electrolysis of molten sodium chloride, a current of $2.50 \text{ A}$ is passed through the cell for $965 \text{ s}$. Calculate the total charge transferred, in coulombs. (Faraday's constant: $F = 96{,}485 \text{ C mol}^{-1}$)

During the electrolysis of molten sodium chloride, chlorine gas is produced at the anode. A constant current of 15.0 A is passed through the cell for 45 minutes. (a) Calculate the charge, in coulombs, that passes through the cell. (1 mark) (b) Calculate the mass of chlorine gas produced, in grams, correct to 3 significant figures. (1 mark) [Given: Faraday's constant = 96,485 C mol\(^{−1}\); molar mass of Cl₂ = 71.0 g mol\(^{−1}\)]