1. THIS IS
Chapter 10
Jeopardy

2. With
Your
Host...
Ms. Siam

3. Jeopardy
Extras
Vocabulary
Vocabulary 2
Heat/q=cmt problems
ΔH problems
Concept Questions
100
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300
300
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400
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4. Entropy
A 100

5. A measure of the disorder of a system

6. Specific heat capacity

7. Energy needed to raise temperature of 1 g of a substance by 1°C

8. Calorie
A 300

9. Energy needed to raise the temperature of 1 g of water by 1 °C

10. Endothermic
A 400

11. Energy as heat flows into system

12. Exothermic
A 500

13. Energy as heat flows out of system

14. Surroundings
B 100

15. The remainder of the universe
B 100

16. System
B 200

17. Portion of the universe in which you are interested
B 200

18. Heat
B 300

19. Flow of energy due to temperature differences
B 300

20. Temperature
B 400

21. Measure of the random motions of molecules and atoms of a substance

22. State function
B 500

23. Property of a system that changes independent of the pathway taken
B 500

24. The amount of energy needed to heat 2. 00 g of carbon from 50
The amount of energy needed to heat 2.00 g of carbon from 50.0°C to 80.0°C is 42.6 J. The specific heat capacity of this sample of carbon is?
C 100

25. 0.710 J/g °C
C 100

26. How many joules of energy would be required to heat 24
How many joules of energy would be required to heat 24.2 g of carbon from 23.6°C to 54.2°C? (Specific heat capacity of carbon = 0.71 J/g °C.)
C 200

27. 5.3 x 102 J
C 200

28. Assume that 372 J of heat is added to 5.00 g of water originally at 23.0°C. What would be the final temperature of the water? (Specific heat capacity of water = J/g °C.)
C 300

29. 40.8°C
C 300

30. Calculate how many calories of heat were added to 177 g of copper as it cooled from 155.0°C to 23.0°C. The specific heat capacity of copper is J/g °C.
C 400

31. 2150 calories
C 400

32. How many calories of heat were added to 5
How many calories of heat were added to 5.0 x 102 g of water to raise its temperature from 25 °C to 55 °C?
C 500

33. 1.5 x 104 calories
C 500

34. (pay attention to the wording “is released”)
When 1 mole of ethylene (C2H4) is burned at constant pressure, 1410 kJ of energy is released as heat. Calculate ΔH for a process in which 10.0 g of ethylene is burned at constant pressure.
(pay attention to the wording “is released”)
D 100

35. -503 kJ
D 100

36. When 1 mole of propane (C3H8) is burned at constant pressure, 2221 kJ of energy is released as heat. Calculate ΔH for a process in which 25.0 g of propane is burned at constant pressure.
D 200

37. -1260 kJ
D 200

38. How much heat is evolved if 25
How much heat is evolved if g of methanol (CH3OH) is burned in excess O2? The reaction is 2CH3OH(l) + 3O2(g)  2CO2(g) + 4H2O(g)
ΔH = kJ
D 300

39. 566.9 kJ
D 300

40. Given the following data: C(s) + O2(g)  CO2(g) ΔH = -393.5kJ
2CO(g)+O2(g)2CO2(g) ΔH = kJ
Calculate ΔH for the reaction
C(s) + 1/2O2(g)  CO(g)
D 400

41. kJ
D 400

42. Given the following data, C(s) + O2(g)  CO2(g) ΔH= -393.5 kJ
C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(l) ΔH= kJ
H2(g) + 1/2O2(g)  H2O(l) ΔH= kJ
Calculate ΔH for the reaction
2C(s) + 2H2(g)  C2H4(g)
D 500

43. 52.3 kJ
D 500

44. A negative sign for the change in enthalpy for a reaction indicates that the reaction is

45. Exothermic
E 100

46. One _____ of water requires 4
One _____ of water requires J of heat to cause a change in temperature of 1°C
E 200

47. Gram
E 200

48. ΔH for a reaction is the ________ of the enthalpy of the products and the enthalpy of the reactants

49. Difference
E 300

50. The amount of heat gained or lost by a substance depends on what three things

51. 1.The change in temperature of the substance
2.The mass of the substance
3.The specific heat capacity of the substance
E 400

52. If a reaction is endothermic, do the reactants or the products of the reaction have the higher potential energy content
E 500

53. Products
E 500

54. Define energy
F 100

55. Ability to do work or produce heat
F 100

56. Define potential energy

57. Stored energy
F 200

58. Define kinetic energy
F 300

59. Energy of motion
F 300

60. Define work
F 400

61. Force acting over a distance

62. If a piece of aluminum of mass 4. 50 g and temperature 99
If a piece of aluminum of mass 4.50 g and temperature 99.5 °C is dropped into 12.0 g of water at 21.0 °C, what will be the final temperature of the water-aluminum mixture? The specific heat capacity of aluminum is J/(g °C)
F 500

63. 26.9 °C
F 500

64. Game Designed By C. Harr-MAIT
Good luck on the test!
Game Designed By C. Harr-MAIT