Consider this two-step mechanism for a reaction: Step 1: NO2(g) + Cl2(g) → ClNO2(g) + Cl(g) Slow Step 2: NO2(g) + Cl(g) → ClNO2(g) Fast c. What is the predicted rate law? a. What is the overall reaction?

Verified step by step guidance

1. <insert step 1> Identify the elementary steps in the given mechanism. Step 1: NO_2(g) + Cl_2(g) \rightarrow ClNO_2(g) + Cl(g) (Slow), Step 2: NO_2(g) + Cl(g) \rightarrow ClNO_2(g) (Fast).
2. <insert step 2> Determine the overall reaction by adding the two elementary steps. Cancel out any intermediates that appear on both sides of the reaction.
3. <insert step 3> Identify the rate-determining step, which is the slowest step in the mechanism. In this case, it is Step 1.
4. <insert step 4> Write the rate law based on the rate-determining step. The rate law is determined by the reactants involved in the slow step.
5. <insert step 5> Express the rate law using the concentrations of the reactants from the slow step: Rate = k[NO_2][Cl_2], where k is the rate constant.>