1. With how much energy must two particles collide for a reaction to occur?

Question 1 of 15

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

Question 2 of 15

3. Large chips of calcium carbonate reacts with an excess of hydrochloric acid 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 a powdered calcium carbonate?

Question 3 of 15

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

Question 4 of 15

5. On a graph showing gas produced (vertical axis) over time (horizontal axis), how does the line tell us the rate of reaction?

Question 5 of 15

6. What is a catalyst?

Question 6 of 15

7. Explain how a catalyst works

Question 7 of 15

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

Question 8 of 15

9. 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 9 of 15

10. Explain the effects of increasing the concentration of solutions on the rate of a reaction in terms of particle collision theory

Question 10 of 15

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

Question 11 of 15

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

Question 12 of 15

13. Write the word equation for the decompostion of hydrogen peroxide, H₂O₂

Question 13 of 15

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

Question 14 of 15

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

Question 15 of 15


 

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