1. One feature of dynamic equilibrium is that the rate of the forward reaction is equal to the rate of the backward reaction. What is the other feature?

Question 1 of 15

2. For a reversible reaction to reach dynamic equilibria, where must the reaction take place?

Question 2 of 15

3. What will happen to the equilibrium position when we decrease temperature? Give a reason for your prediction. A (g) + B (g) ⇋ C (g) + D (g) (+∆H)

Question 3 of 15

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

Question 4 of 15

5. In the thermal decomposition of calcium carbonate, we might expect 50g of calcium carbonate to produce 28g of calcium oxide. If instead only 24g of calcium oxide is produced, what is the percentage yield?

Question 5 of 15

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

Question 6 of 15

7. What does this diagram represent?

Question 7 of 15

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

Question 8 of 15

9. Explain why experimental values of enthalpy change differ from theoretical values

Question 9 of 15

10. Why a catalyst does not affect the position of equilibrium in a reversible reaction?

Question 10 of 15

11. State and explain how increasing temperature affects the diffusion of a gas

Question 11 of 15

12. Ammonia and hydrogen chloride react together in a reversible reaction to produce a white solid. What are the word and symbol equations?

Question 12 of 15

13. What does the symbol ⇌ mean?

Question 13 of 15

14. What is meant by the term exothermic?

Question 14 of 15

15. Describe the chemical test for water

Question 15 of 15


 

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