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1. During the phase change from solid to liquid, the temperature of the sample a) increases

1. During the phase change from solid to liquid, the temperature of the sample a) increases b) decreases c) doubles d) halves e) does not change. a) increases. 2. The process of melting the solid sample is an ________________ process. a) endothermic b) exothermic

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1. During the phase change from solid to liquid, the temperature of the sample a) increases

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  1. 1. During the phase change from solid to liquid, the temperature of the sample a) increases b) decreases c) doubles d) halves e) does not change

  2. a) increases

  3. 2. The process of melting the solid sample is an ________________ process. a) endothermic b) exothermic c) neither, energy is not created nor destroyed

  4. 2. The process of melting the solid sample is an ________________ process. a) endothermic b) exothermic c) neither, energy is not created nor destroyed

  5. 3. During the condensation of the water vapor to water, heat is _________ by the system. a) gained b) lost c) neither

  6. 3. During the condensation of the water vapor to water, heat is _________ by the system. • a) gained • b) lost • c) neither

  7. 4. The vaporization of water is a _______________________ process. a) slow b) exothermic c) endothermic d) boring

  8. 4. The vaporization of water is a _______________________ process. • a) slow • b) exothermic • c) endothermic • d) boring

  9. 5. Which of the following is an exothermic process? a) Candle wax melting b) A puddle evaporating c) Dry ice (solid CO2) subliming to form gaseous CO2 d) Water freezing to form ice

  10. 5. Which of the following is an exothermic process? • a) Candle wax melting • b) A puddle evaporating • c) Dry ice (solid CO2) subliming to form gaseous CO2 • d) Water freezing to form ice

  11. 6. A measure of the average kinetic energy of the particles in a sample of matter is a. heat b. enthalpy c. temperature d. energy e. both

  12. 6. A measure of the average kinetic energy of the particles in a sample of matter is • a. heat • b. enthalpy • c. temperature • d. energy • e. both

  13. 7. As ice cools from 0oC to -10oC, the average kinetic energy of its molecules will ________________________. a. decrease b. increase c. remain the same

  14. 7. As ice cools from 0oC to -10oC, the average kinetic energy of its molecules will ________________________. • a. decrease • b. increase • c. remain the same

  15. 8. Water has a ____________________ specific heat, which allows it to heat and cool slowly. a. high b. low

  16. 8. Water has a ____________________ specific heat, which allows it to heat and cool slowly. • a. high • b. low

  17. 9. Solid X is placed in contact with solid Y. Heat will flow spontaneously from X to Y when _______________________. a. X is 20°C and Y is 20°C b. X is 10°C and Y is 5°C c. X is -25°C and Y is -10°C d. X is 25°C and Y is 30°C

  18. 9. Solid X is placed in contact with solid Y. Heat will flow spontaneously from X to Y when _______________________. • a. X is 20°C and Y is 20°C • b. X is 10°C and Y is 5°C • c. X is -25°C and Y is -10°C • d. X is 25°C and Y is 30°C

  19. 10. Compared to 100 g of iron, a 10-g sample of iron has ____________. a. a higher specific heat b. a lower specific heat c. the same specific heat

  20. 10. Compared to 100 g of iron, a 10-g sample of iron has ____________. • a. a higher specific heat • b. a lower specific heat • c. the same specific heat

  21. 11. When a 37.5 gram sample of an unknown metal cools from 77 ˚C to 23 ˚C, 560 J of energy is released. Find the specific heat capacity of the unknown metal. a) 0.149 J/g˚C b) 2.28 J/g˚C c) 0.277 J/g˚C d) 16.1 J/g˚C

  22. 11. When a 37.5 gram sample of an unknown metal cools from 77 ˚C to 23 ˚C, 560 J of energy is released. Find the specific heat capacity of the unknown metal. • a) 0.149 J/g˚C • b) 2.28 J/g˚C • c) 0.277 J/g˚C • d) 16.1 J/g˚C

  23. 12. How much heat is absorbed when a 15.8 g sample of potassium with c = 0.75 J/g˚C changes temperature by 14˚C? a) 51.7 J b) 165.9 J c) 106.6 J d) 4.245 J

  24. 12. How much heat is absorbed when a 15.8 g sample of potassium with c = 0.75 J/g˚C changes temperature by 14˚C? • a) 51.7 J • b) 165.9 J • c) 106.6 J • d) 4.245 J

  25. 13. A chunk of iron (CFe = 0.46 J/g˚C) at 90˚C is added to a calorimeter containing 150 g of water at 23˚C. The final temperature of the system is 31˚C. What was the mass of the iron? a) 189.1 g b) 1.005 g c) 166.5 g d) 124.0 g

  26. 13. A chunk of iron (CFe = 0.46 J/g˚C) at 90˚C is added to a calorimeter containing 150 g of water at 23˚C. The final temperature of the system is 31˚C. What was the mass of the iron? • a) 189.1 g • b) 1.005 g • c) 166.5 g • d) 124.0 g

  27. 14. A sample of 2.8 grams of water is cooled from 105°C to -6°C. How much heat is lost from the sample? ∆H fusion = 333.5 J/g ∆H vap = 2260 J/g C solid = 2.1 J/g°C C liquid = 4.184 J/g°C C vapor = 1.7 J/g°C a)1299.144 J b)1632.76 J c)2259.04 J d)8492.4 J

  28. 14. A sample of 2.8 grams of water is cooled from 105°C to -6°C. How much heat is lost from the sample? • ∆H fusion = 333.5 J/g • ∆H vap = 2260 J/g • C solid = 2.1 J/g°C • C liquid = 4.184 J/g°C • C vapor = 1.7 J/g°C • a)1299.144 J • b)1632.76 J • c)2259.04 J • d)8492.4 J

  29. 15. A light bulb filament made of tungsten has a mass of 1 g and has a temperature of 1500 C. Calculate the amount of heat released when the filament is cooled to 20 C. The specific heat capacity of tungsten is 0.142 J/g C. a) 210.16 J b) 10563.4 J c) 1500.142 d) 20.142

  30. 15. A light bulb filament made of tungsten has a mass of 1 g and has a temperature of 1500 C. Calculate the amount of heat released when the filament is cooled to 20 C. The specific heat capacity of tungsten is 0.142 J/g C. • a) 210.16 J • b) 10563.4 J • c) 1500.142 • d) 20.142

  31. 16. When natural gas (methane, CH4) is burned, 891.2 kJ of heat is produced as follows: CH4 + 2 O2 ----> CO2 + 2 H2O + 891.2 kJ How much heat will be produced by the burning of 454 grams of natural gas? a) 404604.8 kJ b) 25287.8 kJ c) 1.96 kJ d) 1345.2 kJ

  32. 16. When natural gas (methane, CH4) is burned, 891.2 kJ of heat is produced as follows: • CH4 + 2 O2 ----> CO2 + 2 H2O + 891.2 kJ • How much heat will be produced by the burning of 454 grams of natural gas? • a) 404604.8 kJ • b) 25287.8 kJ • c) 1.96 kJ • d) 1345.2 kJ

  33. 17. When baking soda decomposes, the reaction is 2NaHCO3 (s) ----> Na2CO3 (s) + H2O (g) + CO2 (g) H = 129 kJ Determine the mass of baking soda that will decompose when 65.3 kJ of energy are applied to the system. a) 63.7 g b) 184 g c) 85 g d) 1.98 g

  34. 17. When baking soda decomposes, the reaction is • 2NaHCO3 (s) ----> Na2CO3 (s) + H2O (g) + CO2 (g) H = 129 kJ • Determine the mass of baking soda that will decompose when 65.3 kJ of energy are applied to the system. • a) 63.7 g • b) 184 g • c) 85 g • d) 1.98 g

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