Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) – N2(g) + 2H2O(g) Initial concentrations and rates of reaction are given here. Initial Concentration, [H] (mol/L) Experiment Initial Concentration Initial Rate of Formation of [NO] (mol/L) N2 (mol/L min) 0.0060 0.0010 1.8 x 10-4 0.0060 0.0020 3.6 x 10-4 0.0010 0.0060 0.30 x 10-4 4 0.0020 0.0060 1.2 x 10-4 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO + NO = N,02 Step 2: N202+ H2 = H20+N20 Step 3: N20+H2 = N2+ H20 Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction. 2. 3.

Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) – N2(g) + 2H2O(g) Initial concentrations and rates of reaction are given here. Initial Concentration, [H] (mol/L) Experiment Initial Concentration Initial Rate of Formation of [NO] (mol/L) N2 (mol/L min) 0.0060 0.0010 1.8 x 10-4 0.0060 0.0020 3.6 x 10-4 0.0010 0.0060 0.30 x 10-4 4 0.0020 0.0060 1.2 x 10-4 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO + NO = N,02 Step 2: N202+ H2 = H20+N20 Step 3: N20+H2 = N2+ H20 Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction. 2. 3.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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