a) i) What is meant by the term 'redox reaction'? ii) Using the reaction between iron(III) ions and iodide ions as an example: 2Fe³⁺(aq) + 2I⁻(aq) → 2Fe²⁺(aq) + I₂(aq) Identify the oxidising agent and the reducing agent, showing clearly the change in oxidation number of the relevant species. b) Chlorine gas is passed into a solution of potassium bromide. i) Write a balanced ionic equation for the reaction that occurs. ii) Identify the species oxidised and the species reduced. iii) Using standard electrode potentials below, explain why the reaction is feasible: Cl₂(g)/Cl⁻(aq): E° = +1.36 V Br₂(l)/Br⁻(aq): E° = +1.07 V c) In the electrolysis of dilute sulphuric acid using platinum electrodes: i) Write the half-equation for the reaction at the cathode. ii) Write the half-equation for the reaction at the anode. iii) What volume of oxygen gas (measured at s.t.p.) would be produced if a current of 2.0 A is passed for 32 minutes and 10 seconds? (Faraday constant F = 96,500 C mol⁻¹; molar volume of gas at s.t.p. = 22.4 dm³ mol⁻¹)