a) (i) Define the term 'rate of reaction'. (ii) State THREE factors that affect the rate of a chemical reaction. b) The following data were obtained for the reaction between hydrogen peroxide (H2O2) and iodide ions (I⁻) in acidic solution: H2O2(aq) + 2H⁺(aq) + 2I⁻(aq) → I2(aq) + 2H2O(l) | Experiment | [H2O2] / mol dm⁻³ | [I⁻] / mol dm⁻³ | Initial rate / mol dm⁻³ s⁻¹ | |------------|-------------------|-----------------|------------------------------| | 1 | 0.010 | 0.010 | 1.75 × 10⁻⁴ | | 2 | 0.020 | 0.010 | 3.50 × 10⁻⁴ | | 3 | 0.020 | 0.020 | 7.00 × 10⁻⁴ | (i) Determine the order of reaction with respect to H2O2 and with respect to I⁻. (ii) Write the rate equation for the reaction. (iii) Calculate the value of the rate constant, k, stating its units. c) (i) Explain how a catalyst increases the rate of a reaction. (ii) Give ONE example each of a homogeneous catalyst and a heterogeneous catalyst used in industrial or laboratory processes.