The ionic half-equation for the formation of chlorine gas at the anode during the electrolysis of concentrated sodium chloride solution is:
2Cl−(aq)→Cl2(g)+2e− 2\text{Cl}^-(\text{aq}) \rightarrow \text{Cl}_2(\text{g}) + 2\text{e}^- 2Cl−(aq)→Cl2(g)+2e−In a laboratory simulation of this chlor-alkali process, a total charge of 0.150 faradays0.150\text{ faradays}0.150 faradays is passed through the electrolyte.
Calculate the amount, in moles, of chlorine gas, Cl2\text{Cl}_2Cl2, formed.
Calculate the volume of chlorine gas formed at room temperature and pressure (rtp). [The molar volume of a gas is 24 dm3 mol−124\text{ dm}^3\text{ mol}^{-1}24 dm3 mol−1 at rtp.] Give the unit in your answer.
21 exam-style questions on Edexcel IGCSE Chemistry Electrolysis. Each one has a worked solution and a mark scheme showing where the marks go.