Consider the following reaction: O2(g) + 2 NO(g) 2 NO2(g) (a) The rate law for this reaction is first order in O2(g) and

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Consider the following reaction:
O2(g) + 2 NO(g) 2 NO2(g)
(a) The rate law for this reaction is first order in O2(g) andsecond order in NO(g). What is the rate law for this reaction?
Rate = k [O2(g)] [NO(g)]
Rate = k [O2(g)]2 [NO(g)]
Rate = k [O2(g)] [NO(g)]2
Rate = k [O2(g)]2 [NO(g)]2
Rate = k [O2(g)] [NO(g)]3
Rate = k [O2(g)]4 [NO(g)]
(b) If the rate constant for this reaction at a certaintemperature is 14200, what is the reaction rate when [O2(g)] =0.0219 M and [NO(g)] = 0.0290 M?
Rate = ________M/s.
(c) What is the reaction rate when the concentration of O2(g) isdoubled, to 0.0438 M while the concentration of NO(g) is 0.0290M?
Rate = ________M/s