### Formation of Nitrosyl Chloride Suppose the formation of nitrosyl chloride proceeds by the following mechanism: #### Reaction Steps: - **Step 1:** - **Elementary Reaction:** \( \text{NO} (g) + \text{Cl}_2 (g) \rightarrow \text{NOCl}_2 (g) \) - **Rate Constant:** \( k_1 \) - **Step 2:** - **Elementary Reaction:** \( \text{NOCl}_2 (g) + \text{NO} (g) \rightarrow 2\text{NOCl} (g) \) - **Rate Constant:** \( k_2 \) #### Note: - Suppose \( k_1 \ll k_2 \). This indicates that the first step is much slower than the second. ### Tasks: 1. **Write the balanced chemical equation for the overall chemical reaction.** 2. **Write the experimentally-observable rate law for the overall chemical reaction.** - **Note:** Your answer should not contain the concentrations of any intermediates. - **Rate Law Format:** \( \text{rate} = k \, [\,] \)

### Formation of Nitrosyl Chloride Suppose the formation of nitrosyl chloride proceeds by the following mechanism: #### Reaction Steps: - Step 1: - Elementary Reaction: \( \text{NO} (g) + \text{Cl}_2 (g) \rightarrow \text{NOCl}_2 (g) \) - Rate Constant: \( k_1 \) - Step 2: - Elementary Reaction: \( \text{NOCl}_2 (g) + \text{NO} (g) \rightarrow 2\text{NOCl} (g) \) - Rate Constant: \( k_2 \) #### Note: - Suppose \( k_1 \ll k_2 \). This indicates that the first step is much slower than the second. ### Tasks: 1. Write the balanced chemical equation for the overall chemical reaction. 2. Write the experimentally-observable rate law for the overall chemical reaction. - Note: Your answer should not contain the concentrations of any intermediates. - Rate Law Format: \( \text{rate} = k \, [\,] \)

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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