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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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slide1

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

slide3

2. The process of melting the solid sample is an ________________ process.

a) endothermic

b) exothermic

c) neither, energy is not created nor destroyed

slide4

2. The process of melting the solid sample is an ________________ process.

a) endothermic

b) exothermic

c) neither, energy is not created nor destroyed

slide5

3. During the condensation of the water vapor to water, heat is _________ by the system.

a) gained

b) lost

c) neither

slide6

3. During the condensation of the water vapor to water, heat is _________ by the system.

  • a) gained
  • b) lost
  • c) neither
slide7

4. The vaporization of water is a _______________________ process.

a) slow

b) exothermic

c) endothermic

d) boring

slide8

4. The vaporization of water is a _______________________ process.

  • a) slow
  • b) exothermic
  • c) endothermic
  • d) boring
slide9

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

slide10

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
slide11

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

slide12

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
slide13

7. As ice cools from 0oC to -10oC, the average kinetic energy of its molecules will ________________________.

a. decrease

b. increase

c. remain the same

slide14

7. As ice cools from 0oC to -10oC, the average kinetic energy of its molecules will ________________________.

  • a. decrease
  • b. increase
  • c. remain the same
slide15

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

a. high

b. low

slide16

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

  • a. high
  • b. low
slide17

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

slide18

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
slide19

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

slide20

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
slide21

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

slide22

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
slide23

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

slide24

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
slide25

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

slide26

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
slide27

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

slide28

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
slide29

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

slide30

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
slide31

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

slide32

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
slide33

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

slide34

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