### Determining the Rate Law and Rate ConstantTo determine the rate law and the rate constant of the reaction \(3A + B \rightarrow C + D\), use the following experimental data:| Trial | [A]\(_0\) (mmol L\(^{-1}\)) | [B]\(_0\) (mmol L\(^{-1}\)) | Initial Rate (mmol L\(^{-1}\) s\(^{-1}\)) ||-------|----------------------|----------------------|----------------------------------|| 1 | 0.100 | 0.100 | 6.10 x 10\(^{-2}\) || 2 | 0.113 | 0.100 | 7.79 x 10\(^{-2}\) || 3 | 0.100 | 0.084 | 5.12 x 10\(^{-2}\) |### ExplanationThis table provides the initial concentrations of reactants A and B, along with the initial rate of the reaction for three different trials. By analyzing how changes in the concentrations of A and B affect the reaction rate, you can derive the rate law, which relates the rate of the reaction to the concentrations of the reactants.

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1. Use the following data to determine the rate law and the rate constant of the reaction 3A + B → C + D. Trial [A]o, (mmol L-¹) [B]o, (mmol L-¹) Initial Rate, (mmol L-¹ s¹) 1 0.100 0.100 6.10 x 10-² 2 0.113 0.100 3 0.100 0.084 7.79 x 10-² 5.12 x 10-²

1. Use the following data to determine the rate law and the rate constant of the reaction 3A + B → C + D. Trial [A]o, (mmol L-¹) [B]o, (mmol L-¹) Initial Rate, (mmol L-¹ s¹) 1 0.100 0.100 6.10 x 10-² 2 0.113 0.100 3 0.100 0.084 7.79 x 10-² 5.12 x 10-²

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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Question

### Determining the Rate Law and Rate Constant

To determine the rate law and the rate constant of the reaction \(3A + B \rightarrow C + D\), use the following experimental data:

| Trial | [A]\(_0\) (mmol L\(^{-1}\)) | [B]\(_0\) (mmol L\(^{-1}\)) | Initial Rate (mmol L\(^{-1}\) s\(^{-1}\)) |
|-------|----------------------|----------------------|----------------------------------|
| 1 | 0.100 | 0.100 | 6.10 x 10\(^{-2}\) |
| 2 | 0.113 | 0.100 | 7.79 x 10\(^{-2}\) |
| 3 | 0.100 | 0.084 | 5.12 x 10\(^{-2}\) |

### Explanation

This table provides the initial concentrations of reactants A and B, along with the initial rate of the reaction for three different trials. By analyzing how changes in the concentrations of A and B affect the reaction rate, you can derive the rate law, which relates the rate of the reaction to the concentrations of the reactants.

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