What happens to the following reaction if the pressure is increased? A+B 2C+D More products form. Nothing happens. It shifts to the left. It shifts to the right.
What happens to the following reaction if the pressure is increased? A+B 2C+D More products form. Nothing happens. It shifts to the left. It shifts to the right.
Calculus: Early Transcendentals
8th Edition
ISBN:9781285741550
Author:James Stewart
Publisher:James Stewart
Chapter1: Functions And Models
Section: Chapter Questions
Problem 1RCC: (a) What is a function? What are its domain and range? (b) What is the graph of a function? (c) How...
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![### Chemical Equilibrium and Pressure
**Concept Overview:**
Chemical equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction in a closed system, represented by the following equation:
\[ A + B \leftrightarrow 2C + D \]
**Le Chatelier’s Principle:**
Le Chatelier’s Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change.
**Question:**
What happens to the following reaction if the pressure is increased?
\[ A + B \leftrightarrow 2C + D \]
**Options:**
- O More products form.
- O Nothing happens.
- O It shifts to the left.
- O It shifts to the right.
**Explanation:**
When the pressure of a system at equilibrium is increased, the system will shift towards the side with the fewer gas molecules to reduce the pressure. In the given reaction, we compare the number of moles of gas on each side:
- Reactants side (A + B): 1 + 1 = 2 moles
- Products side (2C + D): 2 + 1 = 3 moles
Since the reactant side has fewer gas molecules (2 moles) compared to the product side (3 moles), increasing the pressure will shift the equilibrium towards the reactants.
Thus, the correct answer is:
- O It shifts to the left.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9cb94819-1a07-4759-acce-f74a7dc351e2%2F184324ba-693c-454c-bff5-ca0c2c547f0d%2Fgwvdnf9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Equilibrium and Pressure
**Concept Overview:**
Chemical equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction in a closed system, represented by the following equation:
\[ A + B \leftrightarrow 2C + D \]
**Le Chatelier’s Principle:**
Le Chatelier’s Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change.
**Question:**
What happens to the following reaction if the pressure is increased?
\[ A + B \leftrightarrow 2C + D \]
**Options:**
- O More products form.
- O Nothing happens.
- O It shifts to the left.
- O It shifts to the right.
**Explanation:**
When the pressure of a system at equilibrium is increased, the system will shift towards the side with the fewer gas molecules to reduce the pressure. In the given reaction, we compare the number of moles of gas on each side:
- Reactants side (A + B): 1 + 1 = 2 moles
- Products side (2C + D): 2 + 1 = 3 moles
Since the reactant side has fewer gas molecules (2 moles) compared to the product side (3 moles), increasing the pressure will shift the equilibrium towards the reactants.
Thus, the correct answer is:
- O It shifts to the left.
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