1. 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 1 of 15

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

Question 2 of 15

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

Question 3 of 15

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

Question 4 of 15

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

Question 5 of 15

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

Question 6 of 15

7. What happens to the rate of reaction if the concentration of solutions is INCREASED?

Question 7 of 15

8. 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 at a higher temperature?

Question 8 of 15

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

Question 9 of 15

10. What is a catalyst?

Question 10 of 15

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

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

Question 13 of 15

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

Question 14 of 15

15. Explain how a catalyst works

Question 15 of 15


 

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