**Title: Determining Rate Laws for Elementary Reactions****Introduction:**This section discusses how to determine the rate law for various elementary reactions by using the rate constant, \( k \).**Reactions and Rate Laws:**1. **Reaction a:** \[ \text{H}_2(g) + \text{O}(g) \rightarrow \text{H}(g) + \text{OH}(g) \] - **Rate Law:** Rate = \( k [\text{H}_2][\text{O}] \)2. **Reaction b:** \[ \text{O}(g) + \text{O}_3(g) \rightarrow 2 \text{O}_2(g) \] - **Rate Law:** Rate = \( k [\text{O}][\text{O}_3] \)3. **Reaction c:** \[ 2 \text{NO}_2(g) \rightarrow \text{N}_2\text{O}_4(g) \] - **Rate Law:** Rate = \( k [\text{NO}_2]^2 \)**Explanation:**In each of these reactions, the rate law is determined by the stoichiometry of the reactants in the elementary reaction. The concentration of each reactant is raised to the power of its stoichiometric coefficient.

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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

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

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**Title: Determining Rate Laws for Elementary Reactions**

**Introduction:**
This section discusses how to determine the rate law for various elementary reactions by using the rate constant, \( k \).

**Reactions and Rate Laws:**

1. **Reaction a:**
\[
\text{H}_2(g) + \text{O}(g) \rightarrow \text{H}(g) + \text{OH}(g)
\]
- **Rate Law:** Rate = \( k [\text{H}_2][\text{O}] \)

2. **Reaction b:**
\[
\text{O}(g) + \text{O}_3(g) \rightarrow 2 \text{O}_2(g)
\]
- **Rate Law:** Rate = \( k [\text{O}][\text{O}_3] \)

3. **Reaction c:**
\[
2 \text{NO}_2(g) \rightarrow \text{N}_2\text{O}_4(g)
\]
- **Rate Law:** Rate = \( k [\text{NO}_2]^2 \)

**Explanation:**
In each of these reactions, the rate law is determined by the stoichiometry of the reactants in the elementary reaction. The concentration of each reactant is raised to the power of its stoichiometric coefficient.

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Elementary reactions are the reactions which occurs in a single step, all the atoms, ions or molecules of the reactants present in the balanced chemical reaction can simultaneously come together in collide with each other .

& the rate of such reaction is proportional to the product of the atoms , ions or molecules of different Reactants raised to their corresponding coefficients.

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