Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Rates of Reaction
164 practice questions
Topics covered
- Experiments to measure the rate of reaction19 practice questions
- Explaining what's happening19 practice questions
- Changing the surface area of the reactants19 practice questions
- Changing the concentration of the reactants19 practice questions
- Changing the pressure on the reaction19 practice questions
- What are catalysts?19 practice questions
- How does a catalyst work?20 practice questions
- Catalysts in industry19 practice questions
Practice questions
1–10 of 68 · Easy
Question 1
1 mark · Easy
Answer and see the solution →State one factor that can be changed to investigate its effect on the rate of a reaction between a solid and a liquid.
Question 2
3 marks · Easy
Answer and see the solution →A student is investigating how the concentration of hydrochloric acid affects the rate of reaction with excess marble chips. The student collects the gas produced during the reaction.
(a)[1 mark]Name the gas produced in this reaction.
(b)[1 mark]State a piece of equipment the student can use to measure the volume of this gas.
(c)[1 mark]Explain why marble chips are added in excess, rather than using the exact amount needed for the acid.
Question 3
2 marks · Easy
Answer and see the solution →In an experiment, a student collects 36 cm³ of carbon dioxide gas in 3 minutes. Calculate the average rate of reaction in cm³/min.
Question 4
2 marks · Easy
Answer and see the solution →Explain how increasing the temperature affects the rate of a reaction between a solid and a solution. Give two reasons for your answer.
Question 5
3 marks · Easy
Answer and see the solution →The table below shows part of an experiment where the mass of carbon dioxide lost was measured every minute as marble chips reacted with dilute hydrochloric acid.
Time / min Mass of CO2 lost / g 0 0.00 1 0.38 2 0.59 3 0.68 4 0.71 (a)[1 mark]Calculate the average rate of reaction between 1 and 2 minutes, giving your answer in g/min.
(b)[1 mark]At which time interval was the reaction fastest? Give your reasoning.
(c)[1 mark]Suggest one practical reason why the mass measured might not decrease exactly as expected.
Question 6
1 mark · Easy
Answer and see the solution →State the name of the solid reactant used in the reaction with hydrochloric acid to produce carbon dioxide gas.
Question 7
3 marks · Easy
Answer and see the solution →A student performs an experiment to investigate how a catalyst affects the rate of decomposition of hydrogen peroxide solution. The student uses different solids as possible catalysts.
(a)[1 mark]State the name of the gas collected during the decomposition of hydrogen peroxide.
(b)[1 mark]Give one method by which the rate of gas production can be measured in this experiment.
(c)[1 mark]Suggest why different solids may produce different rates of reaction.
Question 8
2 marks · Easy
Answer and see the solution →A reaction produces 80 cm³ of carbon dioxide in 4 minutes. Calculate the average rate of reaction in cm³/min.
Question 9
1 mark · Easy
Answer and see the solution →State the minimum condition that must be met for a chemical reaction to occur between two particles, according to collision theory.
Question 10
3 marks · Easy
Answer and see the solution →The reaction between powdered iron and dilute sulfuric acid produces hydrogen gas.
(a)[1 mark]State what particles must do for a reaction to take place according to collision theory.
(b)[1 mark]Name the term for the minimum amount of energy particles need to react when they collide.
(c)[1 mark]Explain why the reaction slows down as the acid is gradually used up.