The reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0500 0.0500 0.0475 2 0.0500 0.100 0.0950 3 0.100 0.0500 0.190 4 0.100 0.100 0.380 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate = k [ClO2(aq)]4 [OH-(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of ClO2(aq) is 0.100 M and that of OH-(aq) is 0.119 M if the temperature is the same as that used to obtain the data shown above? M/s