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
21–30 of 68 · Easy
Question 21
3 marks · Easy
Answer and see the solution →The graph below shows how the mass of carbon dioxide produced changes over time during the reaction between excess hydrochloric acid and two forms of calcium carbonate, both of the same mass.
Graph: Mass of CO2 produced (g) vs. Time (minutes) (a)[1 mark]Which form of calcium carbonate reacts faster? Give evidence from the graph.
(b)[1 mark]State the total mass of carbon dioxide produced at the end of both reactions.
(c)[1 mark]Explain why both forms produce the same final mass of carbon dioxide.
Question 22
1 mark · Easy
Answer and see the solution →Complete the sentence: Reactions between a solid and a liquid are faster when the solid has a ________ surface area.
Question 23
3 marks · Easy
Answer and see the solution →Iron filings (very small pieces) and an iron nail (large piece) are both placed separately into dilute sulfuric acid. The mass of each iron sample is the same.
(a)[1 mark]State which form of iron will react more quickly.
(b)[2 marks]Describe two reasons why the form you selected in (a) reacts faster.
Question 24
2 marks · Easy
Answer and see the solution →A reaction between a solid and a liquid produced 32 cm³ of gas in 4 minutes. When the same mass of solid is powdered and reacted in the same conditions, the reaction is complete in 2 minutes. Calculate the average rate of gas production in both cases. Give your answers in cm³/min and compare the results.
Question 25
1 mark · Easy
Answer and see the solution →State what happens to the rate of a reaction if the concentration of a reactant is increased, assuming all other conditions remain the same.
Question 26
3 marks · Easy
Answer and see the solution →A student dilutes 10.0 cm³ of 2.00 mol/dm³ sodium thiosulfate solution by adding water to make a total volume of 50.0 cm³.
(a)[1 mark]State the formula used to calculate the concentration of the diluted solution.
(b)[2 marks]Calculate the concentration of sodium thiosulfate after dilution.
Question 27
2 marks · Easy
Answer and see the solution →In an experiment, 0.27 g of oxygen gas is produced in 45 seconds during the reaction of hydrogen peroxide with manganese(IV) oxide. Calculate the average rate of oxygen production during this time. Give your answer in g/s.
Question 28
2 marks · Easy
Answer and see the solution →A graph plots the rate of a chemical reaction against the concentration of a reactant. The graph is a straight line that passes through the origin. Explain what this tells you about the relationship between the rate of the reaction and the concentration of the reactant.
Question 29
3 marks · Easy
Answer and see the solution →The table gives the results from an experiment measuring the rate of a reaction at two different concentrations of sulfuric acid.
(a)[0 marks]Concentration of acid (mol/dm³) Rate of reaction (g/s) 0.60 0.008 1.20 0.016 (b)[1 mark]Describe the effect of doubling the concentration on the rate of reaction.
(c)[2 marks]Explain why doubling the concentration causes this effect, in terms of particle collisions.
Question 30
1 mark · Easy
Answer and see the solution →A student mixes 16.0 cm³ of 1.50 mol/dm³ hydrochloric acid with water to make 40.0 cm³ of solution. State the concentration of hydrochloric acid after dilution, leaving your answer as a formula or calculation.