3. Study the two-step reactions below. Reaction 1: Step 1 (slow): H2(g) + ICI(g) → HI(g) + HCI(g) Step 2 (fast): HI(g) + ICI(g) → I2(g) + HCl(g) Reaction 2: Step 1 (slow): NO(g) + NO(g) → N2O2(g) Step 2 (fast): N2O2(g) + O2(g) → 2NO2(g) For each two-step reaction, answer the following: a) Write the over-all reaction. What substance is the reaction intermediate? b) What is the rate law for the mechanism? c) What is the molecularity of the mechanism?

3. Study the two-step reactions below. Reaction 1: Step 1 (slow): H2(g) + ICI(g) → HI(g) + HCI(g) Step 2 (fast): HI(g) + ICI(g) → I2(g) + HCl(g) Reaction 2: Step 1 (slow): NO(g) + NO(g) → N2O2(g) Step 2 (fast): N2O2(g) + O2(g) → 2NO2(g) For each two-step reaction, answer the following: a) Write the over-all reaction. What substance is the reaction intermediate? b) What is the rate law for the mechanism? c) What is the molecularity of the mechanism?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 73QRT

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