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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What shift will this make?
Shift left, shift right or no shift? How do you know?
![### Chemical Equilibrium: The Haber Process
#### Reaction Overview
The Haber process is an industrial method for synthesizing ammonia (NH₃) from nitrogen gas (N₂) and hydrogen gas (H₂). The chemical equilibrium involved in this process can be represented by the following equation:
\[ \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) + \text{heat} \]
This indicates that the formation of ammonia is exothermic, releasing heat.
#### Example Problem: Impact of Adding Ammonia
**Scenario:**
1. **Ammonia (NH₃) is added.**
When ammonia is added to the system, according to Le Chatelier’s Principle, the equilibrium will shift in the direction that opposes the change. In this case:
**Dropdown Choice Explanation:**
- The possible options could include shifting towards reactants, shifting towards products, or no change.
- Select the correct option based on the following principles.
By adding ammonia, the system will seek to reduce the concentration of NH₃ by shifting the equilibrium to the left, favoring the production of nitrogen (N₂) and hydrogen (H₂) and hence absorbing some of the added ammonia.
\[ \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \leftarrow 2\text{NH}_3(\text{g}) + \text{heat} \]
This adjustment helps the system counteract the disturbance and restore a new equilibrium state.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fd17524-060d-4adb-8fd7-51abd298d44d%2Ffe38d3f6-0315-4fb3-b61a-69a34d46b16f%2Fz0xj4fa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium: The Haber Process
#### Reaction Overview
The Haber process is an industrial method for synthesizing ammonia (NH₃) from nitrogen gas (N₂) and hydrogen gas (H₂). The chemical equilibrium involved in this process can be represented by the following equation:
\[ \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) + \text{heat} \]
This indicates that the formation of ammonia is exothermic, releasing heat.
#### Example Problem: Impact of Adding Ammonia
**Scenario:**
1. **Ammonia (NH₃) is added.**
When ammonia is added to the system, according to Le Chatelier’s Principle, the equilibrium will shift in the direction that opposes the change. In this case:
**Dropdown Choice Explanation:**
- The possible options could include shifting towards reactants, shifting towards products, or no change.
- Select the correct option based on the following principles.
By adding ammonia, the system will seek to reduce the concentration of NH₃ by shifting the equilibrium to the left, favoring the production of nitrogen (N₂) and hydrogen (H₂) and hence absorbing some of the added ammonia.
\[ \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \leftarrow 2\text{NH}_3(\text{g}) + \text{heat} \]
This adjustment helps the system counteract the disturbance and restore a new equilibrium state.
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