Answer Happy

The reaction of selenious acid with iodide ions in acidic solution occurs according to the following equation: H₂SeO3(aq) + 6 1 (aq) + 4H+ (aq) → Se (s) + 2 13(aq) + 3 H₂O (1) It was found that the rate of consumption of H₂SeO³ was 2.5 mol dm-3 min-¹ (i) Write the differential rate law for the reaction. (ii) What is the rate of formation of 13? [H2SeO3] M[1]/M [H+]/M Rate / M s-1 Expt. 1 0.644 0.100 0.0413 Expt. 2 0.100 0.100 0.00642 Expt. 3 0.644 0.200 0.165 Expt. 4 0.500 0.200 0.0611 Expt. 5 0.500 0.200 0.173 Table 1. Initial rates data for the reaction of selenious, acid and iodide ions in acidic solution (1 mark) (iii) Initial rates data for the above reaction are given in Table 1 below. Determine the rate law for the reaction, and the rate constant, quoting relevant units. 0.820 0.820 0.820 0.500 1.00 (1 mark)