(a) Write the rate law for the following reactions assuming each reaction fol- lows an elementary rate law. (1) (2) (3) (4) C₂H6C₂H₂ + H₂ C₂H4+20₂ → CH₂ - CH₂ (CH,),COOC(CH;); − C,H+2CH,COCH, nC4H10 iC4H10 (5) CH₂COOC₂H, +C₂H,OH CH3COOCH,+ C₂H5OH
(a) Write the rate law for the following reactions assuming each reaction fol- lows an elementary rate law. (1) (2) (3) (4) C₂H6C₂H₂ + H₂ C₂H4+20₂ → CH₂ - CH₂ (CH,),COOC(CH;); − C,H+2CH,COCH, nC4H10 iC4H10 (5) CH₂COOC₂H, +C₂H,OH CH3COOCH,+ C₂H5OH
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Chapter1: Chemical Foundations
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![**Problem P3-10A: Rate Laws for Elementary Reactions**
For the following chemical reactions, determine the rate law assuming that each reaction proceeds according to an elementary rate law.
**Reactions:**
1. **Reaction 1:**
\[
\text{C}_2\text{H}_6 \rightarrow \text{C}_2\text{H}_4 + \text{H}_2
\]
2. **Reaction 2:**
\[
\text{C}_2\text{H}_4 + \frac{1}{2}\text{O}_2 \rightarrow \overset{O}{\text{CH}_2-\text{CH}_2}
\]
3. **Reaction 3:**
\[
(\text{CH}_3)_3\text{COOC}(\text{CH}_3)_3 \rightleftharpoons \text{C}_2\text{H}_6 + 2\text{CH}_3\text{COCH}_3
\]
4. **Reaction 4:**
\[
n\text{C}_4\text{H}_{10} \rightleftharpoons i\text{C}_4\text{H}_{10}
\]
5. **Reaction 5:**
\[
\text{CH}_3\text{COOC}_2\text{H}_5 + \text{C}_4\text{H}_9\text{OH} \rightleftharpoons \text{CH}_3\text{COO}\text{C}_4\text{H}_9 + \text{C}_2\text{H}_5\text{OH}
\]
**Detailed Explanation:**
Each of the above reactions represents an elementary step, meaning the rate law can be directly written using the stoichiometry of reactants. For an elementary reaction, the rate law is derived from the molecularity of the step:
- **Unimolecular reaction** (e.g., Reaction 1): Rate ∝ [A]
- **Bimolecular reaction** (e.g., Reaction 2): Rate ∝ [A][B]
Understanding elementary reactions forms the basis for more complex reaction mechanisms, where multiple elementary steps combine to describe the overall process.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd47fc2c3-8f4b-4085-b234-bc909be774e3%2F9c1cf1a9-77c4-41da-a587-986fd15cefe3%2Fx0g6fni6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem P3-10A: Rate Laws for Elementary Reactions**
For the following chemical reactions, determine the rate law assuming that each reaction proceeds according to an elementary rate law.
**Reactions:**
1. **Reaction 1:**
\[
\text{C}_2\text{H}_6 \rightarrow \text{C}_2\text{H}_4 + \text{H}_2
\]
2. **Reaction 2:**
\[
\text{C}_2\text{H}_4 + \frac{1}{2}\text{O}_2 \rightarrow \overset{O}{\text{CH}_2-\text{CH}_2}
\]
3. **Reaction 3:**
\[
(\text{CH}_3)_3\text{COOC}(\text{CH}_3)_3 \rightleftharpoons \text{C}_2\text{H}_6 + 2\text{CH}_3\text{COCH}_3
\]
4. **Reaction 4:**
\[
n\text{C}_4\text{H}_{10} \rightleftharpoons i\text{C}_4\text{H}_{10}
\]
5. **Reaction 5:**
\[
\text{CH}_3\text{COOC}_2\text{H}_5 + \text{C}_4\text{H}_9\text{OH} \rightleftharpoons \text{CH}_3\text{COO}\text{C}_4\text{H}_9 + \text{C}_2\text{H}_5\text{OH}
\]
**Detailed Explanation:**
Each of the above reactions represents an elementary step, meaning the rate law can be directly written using the stoichiometry of reactants. For an elementary reaction, the rate law is derived from the molecularity of the step:
- **Unimolecular reaction** (e.g., Reaction 1): Rate ∝ [A]
- **Bimolecular reaction** (e.g., Reaction 2): Rate ∝ [A][B]
Understanding elementary reactions forms the basis for more complex reaction mechanisms, where multiple elementary steps combine to describe the overall process.
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