The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side. Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium. On increasing the pressure, the equilibrium shifts in the direction where the concentration is less. If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

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Answer 1

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Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

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Answer 2

Question

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Expert Solution & Answer

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Answer 4

Question

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 5

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Answer 6

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Answer 7

Chapter 15, Problem 23E

Interpretation Introduction

Interpretation: The effect of increase in pressure of a reaction mixture at equilibrium is to be explained if fewer moles of gas particles are present at the product side as compared to the reactant side.

Concept Introduction: Le Chatelier’s principle states that every chemical reaction tries to minimize the disturbance of equilibrium.

On increasing the pressure, the equilibrium shifts in the direction where the concentration is less.

If the product side has fewer moles of gas particles than the reactant side then the equilibrium will shift in a forward direction.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 15 - Q1. Which change is likely to increase the rate of...Ch. 15 - The equilibrium constants at a fixed temperature...Ch. 15 - Q3. The concentrations of A,B, and C for the...Ch. 15 - Q4. What is the correct expression for the...Ch. 15 - Q5. Consider the reaction between NO and to form...Ch. 15 - Q6. The equilibrium constant for this reaction is...Ch. 15 - Prob. 7SAQ Ch. 15 - Q8. The decomposition of is endothermic. Which...Ch. 15 - Prob. 9SAQ Ch. 15 - Prob. 10SAQ

Solution Summary: The author explains Le Chatelier's principle that every chemical reaction tries to minimize the disturbance of equilibrium by shifting the system in a forward direction.

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