Kinetic data was recorded for a chemical reaction and the graphs below were were produced using the data. Bases off these graphs, determine the overall order of the rate law for this reaction. 120 100 -1 30 0.15 C (A) 2. [V] 41 1/[A] $ 0.1 40 35 20 0 10 20 SO 10 20 10 50 60 30 40 time 10 40 time 30 40 time Select one: a. Impossible to tell from the data given. O b. Second O c. Zero d. None of these. e. First The data in the table below were obtained for the reaction: 2 ClO2(aq) + 2OH(aq) ClO3(aq) + ClO2 (aq) + H20 Experiment Number [CIO2] (M) [OH-] (M) Initial Rate (M/s) 1 0.060 0.030 0.0248 2 0.030 0.00276 0.020 0.020 3 0.090 0.00828 What is the order of the reaction with respect to ClO2? Select one: O 0 2 1 X The rate law for this reaction will take the form rate = K[CIO2)(OH-]". If the order of the reaction with respect to [CIO] is 1, then m = 1. If m = 1 and (CIO) is increased by a factor of 3, then we would expect the initial rate to increase by a factor of 3m = 31 = 3. However, if we look at experiment numbers 1 and 2, where [OH-] is held constant and [CIO,] is increased by a factor of 3, we see that the initial rate value did increase but not by a factor of 3