# Consider the hypothetical reaction A + B +2C → 2 D + 3E In a study of this reaction three experiments were run at the same temperature. The rate is defined as −∆[B]/∆ t . Experiment 1: [A] 0 = 2.0 M [B] 0 = 1.0 × 10 −3 M [C] 0 = 1.0 M [B] (mol/L) Time(s) 2.7 × 10 −4 1.0 × 10 5 1.6 × 10 −4 2.0 × 10 5 1.1 × 10 −4 3.0 × 10 5 8.5 × 10 −5 4.0 × 10 5 6.9 × 10 −5 5.0 × 10 5 5.8 × 10 −5 6.0 × 10 5 Experiment 2: [A] 0 = 1.0 × 10 −2 M [B] 0 = 3.0 M [C] 0 = 1.0 M [A] (mol/L) Time(s) 8.9 × 10 −3 1.0 7.1 × 10 −3 3.0 5.5 × 10 −3 5.0 3.8 × 10 −3 8.0 2.9 × 10 −3 10.0 2.0 × 10 −3 13.0 Experiment 3: [A] 0 = 10.0 M [B] 0 = 5.0 M [C] 0 = 5.0 × 10 −1 M [C] (mol/L) Time(s) 0.43 1.0 × 10 −2 0.36 2.0 × 10 −2 0.29 3.0 × 10 −2 0.22 4.0 × 10 −2 0.15 5.0 × 10 −2 0.08 6.0 × 10 −2 Write the rate law for this reaction, and calculate the value of the rate constant.

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter 11, Problem 111CP
Textbook Problem

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