When the reactant concentration ([A]) is plotted against time for some reaction, a linear plot is observed with a slope of 0.18Mmin1. The initial concentration of A is 0.2M. Based on this, which of the following may be concluded? The reaction is first order. The reaction is second order. The reaction rate is 0.18Mmin1. The halfife is 0.556min. The rate constant is 0.18Mmin1. The overall reaction NO2+COCO2+NO has a rate law of rate =k[NO2]2 at low temperature. Which of the following is consistent with this information? CO2 is a reagent in the rate limiting step. A plausible mechanism is 1. NO2+NO2NO3+NO (slow) 2. NO3+CONO2+CO2 (fast) A plausible mechanism is 1. NO2+NO2NO3+NO (fast equilibrium) 2. NO3+CONO2+CO2 (slow) The rate limiting step must be bimolecular. The overall reaction could be the mechanism. That is, NO2+COCO2+NO is an elementary step