Suppose the decomposition of nitryl chloride proceeds by the following mechanism: no2cl(g)→no2(g)+ cl(g) rate constant: k1cl(g)+no2cl(g)→no2(g)+cl2(g)suppo se also k1≪ k2. that is, the first step is much slower than the second. a. write the balanced chemical equation for the overall chemical reaction. b. write the experimentally-observable rate law for the overall chemical reaction. c. express the rate constant k for the overall chemical reaction in terms of k_1, k_2, and (if necessary) the rate constant k1 and k2 for the reverse of the two elementary reactions in the mechanism.