The reaction O2(g) 2 NO(g) 2 NO2(g) was studied at a certain temperature with the following results: Experiment[O2(g)] (M)[NO(g)] (M)Rate (M/s) 10.01300.01300.0292 20.01300.02600.117 30.02600.01300.0584 40.02600.02600.234 (a) 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) What is the value of the rate constant? (c) What is the reaction rate when the concentration of O2(g) is 0.0225 M and that of NO(g) is 0.0271 M if the temperature is the same as that used to obtain the data shown above? M/s