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1. For the reaction 2A + B + C → products, the law rate takes the form of: r=k [A]"[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law?

1. For the reaction 2A + B + C → products, the law rate takes the form of: r=k [A]"[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law?

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 5RQ
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Rate Law Problems 1. For the reaction 2A +B +C→ products, the law rate takes the form of: r =k [A]M[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law? 2. If 2A +B → C+D+ energy represents a one step reaction. a) Write the rate law. b) How is the initial rate of the reaction affected by the following changes: (i) Tripling the concentration of A (ii) Decreasing the size of the container by ½. 3. Consider the net reaction 3A + 4B → products, the following data were obtained: Initial [A] Initial [B] Initial Rate 10 M/min 40 M/min 10 M/min 90 M/min Experiment 1 2.0 M 4.0 M 2.0 M 6.0 M 4.0 M 2 3 2.0 M 10.0 M 4 4.0 M 4. a) What is the rate law for the reaction 2A+2B → C+D if the following is the reaction mechanism? 2B →E A+E>F+C A+F>D Step #1 (slow) Step #2 (fast) Step #3 (fast) b) Ifk=0.012 liters/mole-min., what is the rate when [A] = 2.0 M and [B] = 4.0 M?
Transcribed Image Text:Rate Law Problems 1. For the reaction 2A +B +C→ products, the law rate takes the form of: r =k [A]M[B]^[C]°. Why aren't the coefficients in the balanced equation always the exponents in the rate law? 2. If 2A +B → C+D+ energy represents a one step reaction. a) Write the rate law. b) How is the initial rate of the reaction affected by the following changes: (i) Tripling the concentration of A (ii) Decreasing the size of the container by ½. 3. Consider the net reaction 3A + 4B → products, the following data were obtained: Initial [A] Initial [B] Initial Rate 10 M/min 40 M/min 10 M/min 90 M/min Experiment 1 2.0 M 4.0 M 2.0 M 6.0 M 4.0 M 2 3 2.0 M 10.0 M 4 4.0 M 4. a) What is the rate law for the reaction 2A+2B → C+D if the following is the reaction mechanism? 2B →E A+E>F+C A+F>D Step #1 (slow) Step #2 (fast) Step #3 (fast) b) Ifk=0.012 liters/mole-min., what is the rate when [A] = 2.0 M and [B] = 4.0 M?
More Rate Law Problems 1. a) Write the rate law for the one step reaction 2NO → N;Oz9). b) If the rate of the disappearance of NO is 0.5 M-min" when the concentration of NO is 2.02 M, find the value of k. c) What is the rate of disappearance of NO if the concentration of NO is 1.0 x 10° M? d) How does the rate change when (NO) is (a) doubled and (b) cut to 1/3? 2. The net reaction A+B+2C → D+E @ 400°C follows the rate law, r=k[A]°[C] a) Complete the blanks in the following table: Experiment [A] [B] mol/L |C) k rate mol/L mol/L mol/L'min 2.0 4.0 2.0 1.0 2 2.0 1.0 b) How may the value of the specific rate constant be increased for the above reaction? 3. If buming of CO [2CO + O2→ 200,], proceeds by the steps: 02 + 20 2C0 + 20 → 2002 If the activation energy is much greater for (1) than (2), what is the rate law? (1) (2) 4. a) What is the rate law for 2A + 3B → 2C + D if the following data is obtained: Experiment [A] mol/L [B] mol/L rate mol/L's 0.11 x 10 1.0 x 10 1.0 x 10 1 0.5 1.5 1.5 2.0 4.0 2.0 2 3 b) Find the value of the specific rate constant.
Transcribed Image Text:More Rate Law Problems 1. a) Write the rate law for the one step reaction 2NO → N;Oz9). b) If the rate of the disappearance of NO is 0.5 M-min" when the concentration of NO is 2.02 M, find the value of k. c) What is the rate of disappearance of NO if the concentration of NO is 1.0 x 10° M? d) How does the rate change when (NO) is (a) doubled and (b) cut to 1/3? 2. The net reaction A+B+2C → D+E @ 400°C follows the rate law, r=k[A]°[C] a) Complete the blanks in the following table: Experiment [A] [B] mol/L |C) k rate mol/L mol/L mol/L'min 2.0 4.0 2.0 1.0 2 2.0 1.0 b) How may the value of the specific rate constant be increased for the above reaction? 3. If buming of CO [2CO + O2→ 200,], proceeds by the steps: 02 + 20 2C0 + 20 → 2002 If the activation energy is much greater for (1) than (2), what is the rate law? (1) (2) 4. a) What is the rate law for 2A + 3B → 2C + D if the following data is obtained: Experiment [A] mol/L [B] mol/L rate mol/L's 0.11 x 10 1.0 x 10 1.0 x 10 1 0.5 1.5 1.5 2.0 4.0 2.0 2 3 b) Find the value of the specific rate constant.
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