Rates of Reaction: Collision Theory and Calculations
This lesson covers the fundamental concepts of reaction rates for Year 11 Chemistry, focusing on collision theory, factors affecting rates, and mathematical calculations of mean rates.
Learning objectives
- Define 'rate of reaction' and identify the units used to measure it.
- Explain how changes in temperature, concentration, and surface area affect the rate using collision theory.
- Calculate the mean rate of a chemical reaction using the relevant formula.
- Describe the role of a catalyst in lowering activation energy.
Lesson plan (60 minutes)
Introduction · 5 min
Do Now: Recall questions on states of matter and chemical changes.
Teaching · 15 min
Teacher-led explanation of Collision Theory and factors affecting rates.
Guided Practice · 10 min
Worked example: Calculating mean rate of reaction from a table of data.
Independent Practice · 20 min
Differentiated worksheet tasks (Support, Core, Stretch).
Plenary · 10 min
8-question multiple choice quiz and self-marking.
Key vocabulary
- Rate of Reaction
- The speed at which a chemical reaction takes place.
- Activation Energy
- The minimum energy that colliding particles must have in order to react.
- Catalyst
- A substance that increases the rate of a reaction without being used up.
- Collision Theory
- The theory that chemical reactions only occur when particles collide with sufficient energy.
- Concentration
- The number of particles in a given volume of solution.
Core worksheet (first questions)
- A reaction produces 8g of gas in 10 seconds. Calculate the mean rate of reaction.
- If 40cm³ of gas is collected in 20 seconds, what is the mean rate?
- Explain why increasing the concentration of a reactant increases the rate of reaction.
- How does a catalyst increase the rate of a reaction?
Quiz (sample)
1. What is the definition of the rate of reaction?
- A. The time it takes for a reaction to stop
- B. The amount of product made in a year
- C. The change in concentration of a reactant or product per unit time
- D. The temperature at which a reaction occurs
2. What is 'activation energy'?
- A. The energy released by a reaction
- B. The minimum energy particles must have to react
- C. The energy required to stop a reaction
- D. The energy of the products minus the reactants
3. Which of the following does NOT increase the rate of reaction?
- A. Increasing temperature
- B. Increasing concentration
- C. Adding a catalyst
- D. Increasing the size of reactant lumps (decreasing surface area)
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