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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Multiple Choice

Consider the reaction below:
CH₄ (g) + F₂ (g) ⇌ CF₄ (g) + HF (g) H = + 38.1 KJ/mol
The following changes will shift the equilibrium to the left except one. Which one would not cause a shift to the left?

Add some CF₄.

Remove some F₂.

Decrease the Temperature.

Decrease the container volume.

Increase the partial pressure of HF.

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Verified step by step guidance

Identify the type of reaction: The given reaction is an endothermic reaction, as indicated by the positive enthalpy change (ΔH = +38.1 kJ/mol). This means that heat is absorbed during the reaction.

Apply Le Chatelier's Principle: This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

Analyze each change: Adding CF4 or increasing the partial pressure of HF will increase the concentration of products, causing the equilibrium to shift to the left to produce more reactants. Removing F2 decreases the concentration of a reactant, also shifting the equilibrium to the left to produce more F2.

Consider the effect of temperature: Decreasing the temperature in an endothermic reaction will shift the equilibrium to the left, as the system will try to produce more heat by favoring the exothermic reverse reaction.

Evaluate the effect of volume change: Decreasing the container volume increases the pressure. According to Le Chatelier's Principle, the equilibrium will shift towards the side with fewer moles of gas. In this reaction, both sides have the same number of moles of gas (2 moles), so a change in volume will not affect the equilibrium position.