The reaction 2 NO2(9) +03(9) N05(9) + O2(9) was studied at a certain temperature with the following results: Experiment [NO2(9)] (M) [Og(9)] (M) Rate (M/s) 0.835 0,835 1.67 1.67 0.835 1.67 0.835 1.67 61600 1.23e+05 1.23e+O5 2.47e+05 (a) What is the rate law for this reaction? Rate - k [NO (9)] (03(9)] O Rate = k [NO2(0)] [0,()] Rate - k[NO2(o) [03()]2 Rate = k [NO2(9)[03(0)12 O Rate = k [NO (9)] [03(9)]3 Rate - k[NO (974 [0,(9)] (b) What is the value the rate constant (c) What is the reaction rate when the concentration of NO2(g) is 1.03 M and that of O3(9) is 2.04 M if the temperature is the same as that used to obtain the data shown above? M/S