The ionic half-equation for the formation of oxygen at the positive electrode during the electrolysis of dilute sulfuric acid is: 2H2O→O2+4H++4e−2\text{H}_2\text{O} \rightarrow \text{O}_2 + 4\text{H}^+ + 4\text{e}^-2H2O→O2+4H++4e−. In one experiment, a charge of 0.0600 faraday0.0600\text{ faraday}0.0600 faraday is passed through the solution.
Calculate the amount, in moles, of oxygen formed.
Calculate the volume of oxygen formed at room temperature and pressure (rtp). [The molar volume of a gas is 24 dm3 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.