1. 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 1 of 15

2. Explain the effects of increasing the temperature on the rate of a reaction in terms of particle collision theory

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

Question 4 of 15

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

Question 5 of 15

6. Describe the laboratory preparation of oxygen from hydrogen peroxide

Question 6 of 15

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

Question 7 of 15

8. Explain how a catalyst works

Question 8 of 15

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

Question 9 of 15

10. What happens to the rate of reaction if a catalyst is added?

Question 10 of 15

11. What happens to the rate of reaction if the temperature is INCREASED?

Question 11 of 15

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

Question 12 of 15

13. What is a catalyst?

Question 13 of 15

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

Question 14 of 15

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

Question 15 of 15


 

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