Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

GOB Chemistry

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

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4:03 minutes

Problem 62a

Textbook Question

For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.
a. C(s) + H₂O(g) ⇌ CO(g) + H₂(g)

Verified step by step guidance

Identify the states of matter for each species in the equilibrium reaction: C(s) is a solid, H2O(g) is a gas, CO(g) is a gas, and H2(g) is a gas. Le Châtelier's principle primarily applies to gases when considering pressure changes.

Count the number of moles of gas on each side of the equilibrium. On the left side, there is 1 mole of gas (H2O(g)), and on the right side, there are 2 moles of gas (CO(g) and H2(g)).

Recall Le Châtelier's principle: When the pressure is increased (by decreasing the volume), the equilibrium will shift in the direction that reduces the total number of gas molecules to counteract the change.

Compare the number of gas molecules on each side. Since the left side has fewer gas molecules (1 mole) than the right side (2 moles), the equilibrium will shift toward the side with fewer gas molecules to reduce pressure.

Conclude that the reaction will shift to the left (toward the reactants) when the pressure is increased by decreasing the volume of the equilibrium mixture.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Châtelier's Principle

Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract that change and restore a new equilibrium. This principle is crucial for predicting how a reaction will respond to changes in concentration, temperature, or pressure.

Equilibrium and Reaction Quotient

In a chemical reaction at equilibrium, the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. The reaction quotient (Q) helps determine the direction in which the reaction will shift when conditions change, allowing us to predict how the system will respond to pressure changes.

Effect of Pressure on Gaseous Reactions

In reactions involving gases, increasing the pressure by decreasing the volume favors the side of the equilibrium with fewer moles of gas. This is because the system will shift to reduce the pressure, thus understanding the mole ratio of gaseous reactants and products is essential for predicting the direction of the shift.

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Related Practice

Textbook Question

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?

C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)

b. Increasing pressure by decreasing volume

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Textbook Question

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?

C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)

c. Allowing CH₄ to escape continuously from the reaction vessel

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Textbook Question

Why do catalysts not alter the amounts of reactants and products present at equilibrium?

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Textbook Question

When the following equilibria are disturbed by increasing the pressure, does the concentration of reaction products increase, decrease, or remain the same?

a. 2 CO₂(g) ⇌ 2 CO(g) + O₂(g)

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Textbook Question

The reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) has ∆H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H₂ in an equilibrium mixture increase or decrease when the temperature is decreased?

The reaction H₂(g) + I₂(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease when

c. A catalyst is added?

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Textbook Question

The reaction H₂(g) + I₂(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease when

b. H2 is removed?

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