consider the following reaction: 2 NO2(g) + O3(g) → N2O5(g) + O2(g)

(a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction?

Rate = k [NO2(g)] [O3(g)]

Rate = k [NO2(g)]2 [O3(g)]

Rate = k [NO2(g)] [O3(g)]2

Rate = k [NO2(g)]2 [O3(g)]2

Rate = k [NO2(g)] [O3(g)]3

Rate = k [NO2(g)]4 [O3(g)]

(b) If the rate constant for this reaction at a certain temperature is 65100, what is the reaction rate when [NO2(g)] = 0.863 M and [O3(g)] = 1.20 M? _____Rate = M/s.

(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.73 M while the concentration of O3(g) is 1.20 M? Rate = ______M/s