Question

Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Identify the intermediates in the mechanism Part C What is the predicted rate law?

Answer 1

Part A:                2NO₂ (g) + Cl₂ (g) ---> 2ClNO₂ (g)

Part B:               Cl is the intermdiate

Part C:               Rate = k[NO₂][Cl₂]              slow step is RDS (Rate determining Step)