Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Two-Step Chemical Reaction Analysis
#### Problem Statement:
Consider the reaction coordinate below for a two-step chemical reaction.
[Insert Reaction Coordinate Diagram Here]
In step 1, compound a reacts to form compound b, and in step 2, compound b reacts to form compound c.
i) Which step is an exothermic reaction?
ii) Label the activation energies in the reaction.
#### Diagram Explanation:
**Reaction Coordinate Diagram:**
- The x-axis represents the Reaction Progress.
- The y-axis represents the Energy level.
The diagram shows a two-step reaction with the following stages:
1. **From compound a to compound b:**
- Starting at point **a** (initial energy level of compound a), the energy increases to a peak, indicating the activation energy required for the reaction.
- After reaching the peak, the energy decreases to point **b** (energy level of compound b).
2. **From compound b to compound c:**
- Starting at point **b**, the energy increases again to another peak.
- After reaching this second peak, the energy decreases further to point **c** (final energy level of compound c).
#### Questions:
**i) Which step is an exothermic reaction?**
- An exothermic reaction is identified by a release of energy, where the final energy level is lower than the initial energy level.
- From the diagram, the reaction from compound **b to c** is exothermic since the energy level decreases from compound b to compound c.
**ii) Label the activation energies in the reaction**
- Activation energy is the energy required to reach the peak from the current energy level.
- For **step 1 (a to b)**: The activation energy is the difference in energy between point **a** and the first peak.
- For **step 2 (b to c)**: The activation energy is the difference in energy between point **b** and the second peak.
By understanding these principles, one can analyze the energetic feasibility and nature of chemical reactions.](https://content.bartleby.com/qna-images/question/5eb56816-160f-4162-a308-b7614955b00c/bff4950a-e462-4a07-9da8-e2d9969cc33e/te2ps16_processed.jpeg)
Transcribed Image Text:### Two-Step Chemical Reaction Analysis
#### Problem Statement:
Consider the reaction coordinate below for a two-step chemical reaction.
[Insert Reaction Coordinate Diagram Here]
In step 1, compound a reacts to form compound b, and in step 2, compound b reacts to form compound c.
i) Which step is an exothermic reaction?
ii) Label the activation energies in the reaction.
#### Diagram Explanation:
**Reaction Coordinate Diagram:**
- The x-axis represents the Reaction Progress.
- The y-axis represents the Energy level.
The diagram shows a two-step reaction with the following stages:
1. **From compound a to compound b:**
- Starting at point **a** (initial energy level of compound a), the energy increases to a peak, indicating the activation energy required for the reaction.
- After reaching the peak, the energy decreases to point **b** (energy level of compound b).
2. **From compound b to compound c:**
- Starting at point **b**, the energy increases again to another peak.
- After reaching this second peak, the energy decreases further to point **c** (final energy level of compound c).
#### Questions:
**i) Which step is an exothermic reaction?**
- An exothermic reaction is identified by a release of energy, where the final energy level is lower than the initial energy level.
- From the diagram, the reaction from compound **b to c** is exothermic since the energy level decreases from compound b to compound c.
**ii) Label the activation energies in the reaction**
- Activation energy is the energy required to reach the peak from the current energy level.
- For **step 1 (a to b)**: The activation energy is the difference in energy between point **a** and the first peak.
- For **step 2 (b to c)**: The activation energy is the difference in energy between point **b** and the second peak.
By understanding these principles, one can analyze the energetic feasibility and nature of chemical reactions.
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