1. Instructions for using this template.
Remember this is Jeopardy, so where I have written “Answer” this is the prompt the students will see, and where I have “Question” should be the student’s response.
To enter your questions and answers, click once on the text on the slide, then highlight and just type over what’s there to replace it. If you hit Delete or Backspace, it sometimes makes the text box disappear.
When clicking on the slide to move to the next appropriate slide, be sure you see the hand, not the arrow. (If you put your cursor over a text box, it will be an arrow and WILL NOT take you to the right location.)

2. You will be given the answer. You must give the correct question.
Jeopardy
Choose a category.
You will be given the answer.
You must give the correct question.
Click to begin.

3. Click here for Final Jeopardy
Choose a point value.
Choose a point value.
Click here for Final Jeopardy

4. Factors for
rates of
reactions
Potential
Energy
Diagrams
Equilibrium
Le Chatelier’s
Principle
Entropy and
Enthalpy
10 Point
10 Point
10 Point
10 Point
10 Point
20 Points
20 Points
20 Points
20 Points
20 Points
30 Points
30 Points
30 Points
30 Points
30 Points
40 Points
40 Points
40 Points
40 Points
40 Points
50 Points
50 Points
50 Points
50 Points
50 Points

5. Why does powdered zinc react faster than a strip of zinc

6. More surface area

7. How would an increase in pressure effect the rate of a reaction

8. Increases

9. If less reactant is added in a reaction what effect will this have on the rate of reaction

10. Decrease

11. Between ionic and covalent compounds which will react faster and why

12. Ionic because they are smaller and less bonds to break and form new compounds

13. How does a catalyst effect a reaction?

14. Provides a new pathway or lowers activation energy

15. Which Letter represents the activation energy of the reaction?

16. A

17. Which letter Represents the energy of the products

18. C

19. Calculate the cchange in heat for the reaction

20. 80 kJ

21. What is the activation energy without a catalyst?

22. 140kJ

23. Is the following reaction endo or exothermic? Explain your answer

24. Exothermic because the products have less energy than the reactants

25. What type of equilibrium is shown above
H2O (s) H2O (l)
What type of equilibrium is shown above

26. Phase equilibrium

27. At what temperature will this phase equilibrium occur
H2O (s) H2O (l)
At what temperature will this phase equilibrium occur

28. Zero degrees Celsius

29. What type of solution needs to be present in order to have equilibrium

30. Saturated

31. Compared to the amount of product made the amount of reactant made during equilibrium is….

32. The same

33. In chemical equilibrium if 3 moles of products are produced how many moles of reactant are produced

34. 3 moles

35. 4NH3(g) + SO2(g) 4NO(g) + 6H2O(g)+ heat
In the reaction above if H2O is added to the system which way will it shift

36. Left

37. If heat is added to the system which way will it shift?
4NH3(g) + SO2(g)4NO(g) + 6H2O(g)+heat
If heat is added to the system which way will it shift?

38. Left

39. 4NH3(g) + SO2(g)4NO(g) + 6H2O(g)+heat
If the pressure was decreased in the system which way would the reaction shift?

40. Right

41. 4NH3(g) + SO2(g)4NO(g) + 6H2O(g)+heat
If the concentration of SO2 was increased which way would the reaction shift?

42. right

43. How could more product be produced
X + Y  Z + heat
How could more product be produced

44. Increase concentration of x or y, decrease the heat used

45. Nature tends to move towards what type of entropy

46. high

47. Nature moves towards what type of enthalpy

48. Low

49. Which type of reaction will happen more readily exo or endo?
Explain

50. Exo releases heat lower enthalpy

51. Gas moves from high concentration to lower concentration explain why?

52. To create more entropy (randomness)

53. What conditions must be present for a reaction to happen spontaneously

54. Exothermic and high entropy

55. Final Jeopardy
Make your wager

56. Write the equilibrium equation for the following reaction
H2(g) + F2(g) 2HF(g)

57. Keq=[HF]2/[H2]x[F2]