1. What is meant by the term activation energy?

Question 1 of 15

2. What simple change could be made to a reaction to speed it up dramatically?

Question 2 of 15

3. Explain the effects of increasing the pressure of gases on the rate of a reaction in terms of particle collision theory

Question 3 of 15

4. State the catalyst used for making oxygen through the decomposition of hydrogen peroxide

Question 4 of 15

5. Give a simple reaction can be used to investigate the effect of changing concentration on the rate of reaction

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6. What type of substance speeds up a chemical reaction but is chemically unchanged at the end of the reaction?

Question 6 of 15

7. Give a simple reaction can be used to investigate the effect of changing surface area on the rate of reaction

Question 7 of 15

8. What reactant is used to produce a sample of oxygen in the lab?

Question 8 of 15

9. What happens to the rate of reaction if the surface area of a solid is INCREASED?

Question 9 of 15

10. What is a catalyst?

Question 10 of 15

11. Explain how a catalyst works

Question 11 of 15

12. Explain the effects of increasing the surface area of a solid on the rate of a reaction in terms of particle collision theory

Question 12 of 15

13. What happens if two particles collide with less than the activation energy

Question 13 of 15

14. Hydrochloric acid reacts with an excess of calcum carbonate in a flask. The volume of carbon dioxide given off is measured in a gas syringe. This is shown on the graph. How would the graph look different if the reaction was done with the same volume of acid, but with an acid which is twice as concentrated?

Question 14 of 15

15. Calcium carbonate reacts with an excess of hydrochloric acid in a flask. The mass of flask and contents decreases over time as the carbon dioxide escapes. This is shown on the graph. How would the graph look different if the reaction was done with a lower concentration of hydrochloric acid?

Question 15 of 15