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Chapter 10 Jeopardy: Heat and Entropy Questions with Ms. Siam

Test your knowledge of heat and entropy concepts with this Jeopardy-style game hosted by Ms. Siam. Answer questions on specific heat capacity, enthalpy, system and surroundings, and more.

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Chapter 10 Jeopardy: Heat and Entropy Questions with Ms. Siam

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Presentation Transcript

  1. THIS IS Chapter 10 Jeopardy

  2. Your With Host... Ms. Siam

  3. Jeopardy Extras Vocabulary Vocabulary 2 Heat/q=cmt problems ΔH problems Concept Questions 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

  4. Entropy A 100

  5. A measure of the disorder of a system A 100

  6. Specific heat capacity A 200

  7. Energy needed to raise temperature of 1 g of a substance by 1°C A 200

  8. Calorie A 300

  9. Energy needed to raise the temperature of 1 g of water by 1 °C A 300

  10. Endothermic A 400

  11. Energy as heat flows into system A 400

  12. Exothermic A 500

  13. Energy as heat flows out of system A 500

  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 B 400

  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 50.0°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 24.2 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 = 4.184 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 0.385 J/g °C. C 400

  31. 2150 calories C 400

  32. 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. 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 25.00 g of methanol (CH3OH) is burned in excess O2? The reaction is 2CH3OH(l) + 3O2(g)  2CO2(g) + 4H2O(g) ΔH = -1453 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 = -566.0 kJ Calculate ΔH for the reaction C(s) + 1/2O2(g)  CO(g) D 400

  41. -110.5 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= -1410.9 kJ H2(g) + 1/2O2(g)  H2O(l) ΔH= -285.8 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 E 100

  45. Exothermic E 100

  46. One _____ of water requires 4.184 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 E 300

  49. Difference E 300

  50. The amount of heat gained or lost by a substance depends on what three things E 400

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