JEOPARDY!

1. JEOPARDY! Click Once to Begin Chemistry 7 Final Review By: Catherine Flanagan

2. JEOPARDY! Vocabulary Endothermic and Exothermic Calorimetryand Heat Capacity Practice Problems Enthalpy And Hess’s Law Change in State 100 100 100 100 100 100 200 200 200 200 200 200 300 300 300 300 300 300 400 400 400 400 400 400 500 500 500 500 500 500

3. Vocabulary: 100 Define endothermic

4. A Chemical reaction during which energy is transferred from the surroundings to the system

5. Vocabulary: 200 If the ΔH is negative is it an endothermic or exothermic process?

6. Exothermic

7. Vocabulary: 300 What does a calorie measure?

8. The amount of energy it takes a certain substance to raise 1 gram of water 1 degree Celsius.

9. Vocabulary: 400 What the difference between a calorie and Calorie?

10. A Calorie is 1000 calories.

11. Vocabulary: 500 What is enthalpy of fusion?

12. The amount of heat required to melt 1g of a substance (Hfus).

13. Endothermic and Exothermic: 100 If NH3NO3 is dissolved in water and the temperature decreases is the process endothermic or exothermic?

14. Endothermic

15. Endothermic and Exothermic: 200 Give an example of an exothermic phase change

16. Making iceCondensing water

17. Endothermic and Exothermic: 300 Give an example of an endothermic phase change

18. Boiling or melting water

19. Endothermic and Exothermic: 400 If ΔH is negative the reaction is…

20. Exothermic

21. Endothermic and Exothermic: 500 An ice pack would be a …….. reaction

22. Endothermic

23. Calorimetry and Heat Capacity: 100 Convert 452J to calories

24. 108 calories

25. Calorimetry and Heat Capacity: 200 Convert 384 kJ to calories.

26. 91866 calories

27. Calorimetry and Heat Capacity: 300 If a 10.0g solid is dissolved in a 25.3°C sample of water and the final temperature is 27.4°C What is the value of ΔH? (Cp=.874 J/g°C)

28. ΔH= 18.40 J

29. Calorimetry and Heat Capacity: 400 If 3.4 mol of Aluminum is dissolved in water and the temperature changes from 25°C to 318°K and the specific heat is .874J/g°C What is the ΔH value?

30. ΔH= 1590.70 J

31. Calorimetry and Heat Capacity: 500 How many Calories in 4500 kJ?

32. 94 Calories

33. Practice Problems: 100 Convert 14.7 Calories to Joules

34. 61446 J

35. Practice Problems: 200 If 1520 J are added to 24.5g of water at 63.1°C what will the final temperature be?

36. 77.9°C

37. Practice Problems: 300 45.8g of an unknown substance at 85.4°C is placed in 67.9g of water at 16.1°C, and the final temperature of the system is 22.7°C what is the specific heat capacity of the substance?

38. Cp= .156 cal/g°C

39. Practice Problems: 400 If you dissolve 3g of an unknown substance and the temperature changes 32°C and 56J are produced what is the specific heat?

40. .583J/g°C

41. Daily Double!!! Practice Problems: 500 Given the following information about water:Enthalpy of fusion: 80.87 cal/gSpecific heat of ice: .51 cal/g°CSpecific heat of water: 1cal/g°CSpecific heat of steam: .48 cal/g°CEnthalpy of vaporization: 547.2cal/gHow many calories are needed to warm 53.7g of water at -36.7°C to 136°C?

42. 35779.25 cal

43. Enthalpy and Hess’s Law: 100 Define enthalpy

44. Heat when pressure is held constant

45. Enthalpy and Hess’s Law: 200 What is the value for ΔH for the following reaction?CS2(l) + 2 O2(g) → CO2(g) + 2 SO2(g) Given:C(s) + O2(g) → CO2(g); ΔHf = -393.5 kJ/molS(s) + O2(g) → SO2(g); ΔHf = -296.8 kJ/molC(s) + 2 S(s) → CS2(l); ΔHf = 87.9 kJ/mol

46. -1075.0 kJ/mol.

47. Enthalpy and Hess’s Law: 300 If you want to warm 4.5g of water from 34.6°C to 62.1°C how many joules would you need to add to the water? (Specific heat of water= 4.18)

48. 517.3 J

49. Enthalpy and Hess’s Law: 400 What mass of antimony can you melt with 9451J if the heat of fusion is 165J/g ?

50. 57.30g