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

Rate of Reaction

GOB Chemistry

7. Energy, Rate and Equilibrium

Rate of Reaction

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3:08 minutes

Problem 75a

Textbook Question

How would each of the following change the rate of the reaction shown here? 2SO₂(g) + O₂(g) → 2SO₃(g)
a. adding more SO₂(g)

Verified step by step guidance

Understand the reaction: The given reaction is 2SO₂(g) + O₂(g) → 2SO₃(g). This is a chemical equilibrium reaction where the rate of reaction depends on the concentration of reactants and products.

Identify the factor being changed: In this case, the problem asks about the effect of adding more SO₂(g), one of the reactants.

Apply the principle of concentration and reaction rate: According to the collision theory, increasing the concentration of a reactant (SO₂ in this case) increases the frequency of collisions between reactant molecules, which can increase the rate of the forward reaction.

Consider Le Chatelier's Principle: Adding more SO₂(g) shifts the equilibrium position to favor the formation of products (SO₃), as the system tries to counteract the change by consuming the added SO₂.

Conclude the effect: Adding more SO₂(g) will increase the rate of the forward reaction initially, and over time, the system will adjust to a new equilibrium with more SO₃ formed.

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Key Concepts

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

Reaction Rate

The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be influenced by various factors, including concentration, temperature, and the presence of catalysts. Understanding how these factors affect the reaction rate is crucial for predicting how changes in conditions will impact the overall reaction.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system shifts in a direction that counteracts the change. In the context of the given reaction, adding more SO₂ would shift the equilibrium to the right, favoring the production of SO₃, thereby increasing the rate of the reaction.

Concentration Effects

Concentration effects refer to how the amount of reactants or products in a reaction mixture influences the rate of reaction. Increasing the concentration of a reactant, such as SO₂, typically leads to more frequent collisions between reactant molecules, which can enhance the reaction rate. This principle is fundamental in chemical kinetics and reaction dynamics.

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