The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.835 0.835 47900 2 0.835 1.67 95800 3 1.67 0.835 95800 4 1.67 1.67 1.92e+05 (a) What is the rate law for this reaction? A) Rate = k [NO2(g)] [O3(g)] B) Rate = k [NO2(g)]2 [O3(g)] C) Rate = k [NO2(g)] [O3(g)]2 D) Rate = k [NO2(g)]2 [O3(g)]2 E) Rate = k [NO2(g)] [O3(g)]3 F) Rate = k [NO2(g)]4 [O3(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of NO2(g) is 0.842 M and that of O3(g) is 1.82 M if the temperature is the same as that used to obtain the data shown above?