Consider the following system at equilibrium at 500 K: PCI 3(g) + Cl₂(g) =PC15(g) When some Cl₂(g) is removed from the equilibrium system at constant temperature: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The reaction must: The concentration of PCl3 will: A. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium at 500 K: PCI 3(g) + Cl₂(g) =PC15(g) When some Cl₂(g) is removed from the equilibrium system at constant temperature: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The reaction must: The concentration of PCl3 will: A. Increase. B. Decrease. C. Remain the same.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Could someone explain to me a little better. Its like I am reading it but defently not understanding it
![**Equilibrium and Le Chatelier's Principle**
Consider the following system at equilibrium at 500 K:
\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]
When some \(\text{Cl}_2(g)\) is removed from the equilibrium system at constant temperature:
**The reaction must:**
- A. Run in the forward direction to reestablish equilibrium.
- B. Run in the reverse direction to reestablish equilibrium.
- C. Remain the same. Already at equilibrium.
**The concentration of \(\text{PCl}_3\) will:**
- A. Increase.
- B. Decrease.
- C. Remain the same.
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Transcribed Image Text:**Equilibrium and Le Chatelier's Principle**
Consider the following system at equilibrium at 500 K:
\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]
When some \(\text{Cl}_2(g)\) is removed from the equilibrium system at constant temperature:
**The reaction must:**
- A. Run in the forward direction to reestablish equilibrium.
- B. Run in the reverse direction to reestablish equilibrium.
- C. Remain the same. Already at equilibrium.
**The concentration of \(\text{PCl}_3\) will:**
- A. Increase.
- B. Decrease.
- C. Remain the same.
---
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![LeChatelier's Principle:
A change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner as to reduce or counteract the effect of the change.
Factors that determine the equilibrium conditions of a system are:
1. Concentration
2. Temperature
3. Volume (Pressure) for gaseous systems.
**Concentration**
When a system is at equilibrium, the rate of the reaction in the forward direction is equal to the rate of the reaction in the reverse direction. Changing the concentration of reactants or products disturbs this balance, and the system will seek to restore itself to a new equilibrium that offsets the change.
For example: **Adding reactant** to an equilibrium system.
\[ 2 \text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) \]
Adding \(\text{NO}_2(g)\) will cause the reaction to run in the forward direction to consume the added reactant. Since the rate in the forward direction is temporarily larger than the rate in the reverse direction, reactant will be converted to product to reestablish equilibrium. Therefore, the concentration of \(\text{N}_2\text{O}_4(g)\) will increase.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0ffec19-af41-4c50-af1b-66e883fc2bb8%2F7de8113a-baf5-4341-a443-b966d518198c%2Ftylcdsr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:LeChatelier's Principle:
A change in any of the factors that determine the equilibrium conditions of a system will cause the system to change in such a manner as to reduce or counteract the effect of the change.
Factors that determine the equilibrium conditions of a system are:
1. Concentration
2. Temperature
3. Volume (Pressure) for gaseous systems.
**Concentration**
When a system is at equilibrium, the rate of the reaction in the forward direction is equal to the rate of the reaction in the reverse direction. Changing the concentration of reactants or products disturbs this balance, and the system will seek to restore itself to a new equilibrium that offsets the change.
For example: **Adding reactant** to an equilibrium system.
\[ 2 \text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) \]
Adding \(\text{NO}_2(g)\) will cause the reaction to run in the forward direction to consume the added reactant. Since the rate in the forward direction is temporarily larger than the rate in the reverse direction, reactant will be converted to product to reestablish equilibrium. Therefore, the concentration of \(\text{N}_2\text{O}_4(g)\) will increase.
Expert Solution
Step 1
We are given a reaction at equilibrium,
PCl3 + Cl2 ⇌ PCl5
We are to discuss the effect of removing a few amount of Cl2 from the equilibrium, and explain Le Chatelier's principle.
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