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?
2 SO₂(g) + O₂(g) → 2 SO₃(g)
a. adding some SO₂(g)

Verified step by step guidance

Understand the concept: The rate of a chemical reaction depends on factors such as concentration, temperature, surface area, and the presence of a catalyst. In this case, adding more SO₂(g) affects the concentration of a reactant.

Identify the relationship between concentration and reaction rate: According to the collision theory, increasing the concentration of a reactant increases the frequency of collisions between reactant molecules, which can increase the reaction rate.

Apply the principle to the given reaction: The reaction involves SO₂(g) and O₂(g) as reactants. Adding more SO₂(g) increases its concentration, which leads to more frequent collisions between SO₂(g) and O₂(g) molecules.

Relate this to the rate of reaction: With more frequent collisions, the likelihood of effective collisions (those that result in product formation) also increases, thereby increasing the rate of the reaction.

Conclude: Adding SO₂(g) increases the concentration of one of the reactants, which in turn increases the rate of the reaction according to the collision theory.

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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. In this case, the rate of the reaction can be affected by the concentration of SO₂, as increasing the amount of a reactant typically leads to a higher frequency of collisions between molecules, thus accelerating the reaction.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of the given reaction, adding more SO₂ will shift the equilibrium position to the right, favoring the formation of SO₃, thereby increasing the rate of the reaction until a new equilibrium is established.

Concentration Effects

Concentration effects refer to how the amount of reactants or products in a reaction mixture influences the reaction rate. Increasing the concentration of a reactant, such as SO₂ in this case, leads to more molecules available for reaction, which increases the likelihood of collisions and thus enhances the rate of reaction. This principle is fundamental in understanding how varying concentrations can impact chemical kinetics.

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