Free Printable [Summary] Thermal Properties

Free Printable Worksheets

Worksheets

[Summary] Thermal Properties

Total questions: 70

Worksheet time: 1hrs 6mins

Name

Class

Date

1.

As the thermal energy of matter ___________, its particles usually spread out.

a)

increases

b)

decreases

2.

The change from a gas to a liquid is called

a)

condensation

b)

evaporation

c)

sublimation

d)

deposition

3.

What is Thermal expansion?

a)

The transfer of thermal energy between materials by the collisions of particles

b)

Is a decrease in a materials volume when temperature decreases

c)

An increase in a materials volume when temperature increases

d)

Chicken fried rice

4.

Internal energy consists of

a)

thermal energy and kinetic energy

b)

thermal energy and potential energy

c)

kinetic energy and potential energy

d)

thermal energy, kinetic energy and potential energy

5.

When a substance is heated from 25 ^oC to 50 ^oC,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

6.

When a substance is cooled from 40 ^oC to 10 ^oC,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

7.

When a substance is freezing,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

8.

When a substance is boiling,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

9.

When a substance is melting,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

10.

When a substance is condensing,

a)

its kinetic energy decreases.

b)

its potential energy decreases.

c)

its kinetic energy increases.

d)

its potential energy increases.

11.

When a substance is cooled from gas to liquid,

a)

both its potential energy and internal energy decrease.

b)

both its potential energy and internal energy increase.

c)

its potential energy increases but internal energy decreases.

d)

its potential energy decreases but internal energy increases

12.

When a substance is heated from liquid to gas,

a)

both its potential energy and internal energy decrease.

b)

both its potential energy and internal energy increase.

c)

its potential energy increases but internal energy decreases.

d)

its potential energy decreases but internal energy increases

13.

When the temperature of a liquid increases,

a)

both its kinetic energy and internal energy decrease.

b)

both its kinetic energy and internal energy increase.

c)

its kinetic energy increases but internal energy decreases.

d)

its kinetic energy decreases but internal energy increases

14.

When the temperature of a gas decreases,

a)

both its kinetic energy and internal energy decrease.

b)

both its kinetic energy and internal energy increase.

c)

its kinetic energy increases but internal energy decreases.

d)

its kinetic energy decreases but internal energy increases

15.

When the temperature of a solid decreases,

a)

both its kinetic energy and potential energy decrease.

b)

both its kinetic energy and potential energy increase.

c)

its kinetic energy increases but potential energy remains the same.

d)

its kinetic energy decreases but potential energy remains the same.

16.

When water becomes ice,

a)

its potential energy increases but kinetic energy remains the same.

b)

its potential energy decreases but kinetic energy remains the same.

c)

its kinetic energy increases but potential energy remains the same.

d)

its kinetic energy decreases but potential energy remains the same.

17.

What happens to the molecules in a liquid as it gets hotter?

a)

speed up

b)

slow down

c)

stay at same speed

18.

Phase change from water vapour to liquid water is __________

a)

Fusion

b)

Condensation

c)

Vaporisation

19.

When water reaches its boiling point, the thermal energy will be used to...

a)

raise the temperature of the water above 100^o C

b)

change the liquid particles to gas

c)

add more water particles

d)

slow down the water particles

20.

When a substance changes from a liquid to a solid (freezes), it must...

a)

gain thermal energy

b)

lose thermal energy

21.

When water reaches its boiling point, the thermal energy will be used to...

a)

raise the temperature of the water above 100^o C

b)

change the liquid particles to gas

c)

add more water particles

d)

slow down the water particles

22.

A substance loses thermal energy to the surroundings at a steady rate. The graph shows how the temperature of the substance changes with time. What could the portion PQ of the graph represent?

a)

gas condensing

b)

gas cooling

c)

liquid cooling

d)

liquid solidifying

23.

What causes the random, zig-zag movement (Brownian motion) of smoke particles suspended in air?

a)

air molecules colliding with smoke particles

b)

convection currents as the hot smoke rises

c)

smoke particles colliding with each other

d)

smoke particles reacting with oxygen molecules in the air

24.

Which statement describes what happens as ice at 0°C starts to melt to become water?

a)

Energy is absorbed and the temperature remains constant.

b)

Energy is absorbed and the temperature rises.

c)

Energy is released and the temperature remains constant.

d)

Energy is released and the temperature rises.

25.

A liquid at room temperature fills a flask and a glass tube to level X. The flask is now placed in ice, and the liquid level in the tube falls to level Y. Why does the level fall?

a)

The flask contracts.

b)

The flask expands.

c)

The liquid contracts.

d)

The liquid expands.

26.

Evaporation takes place at any temperature

a)

True

b)

False

27.

Evaporation happens

a)

throughout the liquid

b)

at the surface of a liquid

28.

Define evaporation.

a)

A process in which liquid changes to gas over a range of temperature.

b)

A process in which liquid changes to gas at a fixed temperature.

c)

A process in which water changes to water vapour over a range of temperature.

d)

A process in which water changes to water vapour at a fixed temperature.

29.

Which of the following statements is true when a pot of water is boiling?

a)

Evaporation does not occur during boiling.

b)

Evaporation also happens during boiling.

c)

Bubbles are produced only on the surface of the water.

d)

When bubbles are seen, the temperature of water must be above 100^oC.

30.

Four containers, A, B, C and D, contain equal amounts of water. Fans are blowing at the same speed on top of the containers as shown. Which container will have the most amount of water left after some time?

a)

container A

b)

container B

c)

container C

d)

container D

31.

Four glasses, P, Q, R and S, contain equal amounts of water.

Heating lamps are placed on top of the four glasses as shown.

Which glass will have the least amount of water after some time?

a)

glass P

b)

glass Q

c)

glass R

d)

glass S

32.

Four different containers, A, B, C and D, contain equal amounts of water.

Which container will be the last to dry up?

a)

container A

b)

container B

c)

container C

d)

container D

33.

Four containers, A, B, C and D, contain equal amounts of water. Fans and heating lamps are turned on as shown. Which container will have the most amount of water left after some time?

a)

container P

b)

container Q

c)

container R

d)

container S

34.

How does blowing bubbles into the water increase the rate of evaporation?

a)

increases the exposed surface area of water

b)

increases the temperature of the water

c)

decreases the exposed surface area of water

d)

decreases the temperature of the water

35.

Four sets of wet sponges are shown below.

Which set will dry up first?

a)

set A

b)

set B

c)

set C

d)

set D

36.

The three containers contain same amount of water at different temperatures.

In which container(s) does/do evaporation occur?

a)

Container B only.

b)

Containers A and B only.

c)

Containers B and C only.

d)

Containers A, B and C.

37.

The pouring of water from one cup to another will cause the water to evaporate faster because _________.

a)

the exposed surface of the water increases

b)

the temperature of water increases

c)

the temperature of water decreases

d)

the exposed surface of the water decreases

38.

During evaporation, water molecules on the surface of water ___________________ from the surroundings to move faster and then escape into the air.

a)

absorb energy

b)

lose energy

c)

share energy

39.

Liquid evaporates from a beaker.

What happens to the temperature of the remaining liquid and why?

a)

temperature decreases, because the average KE of the particles reduced.

b)

temperature decreases because the particles are now in constant random motion.

c)

temperature increases because the remaining particles have more space and hence move faster.

d)

temperature increases because the energy from the surroundings increases convection.

40.

Which liquid will evaporate the fastest?

a)

olive oil

b)

nail-polish remover

c)

vinegar

41.

The ________________ of a substance is the amount of energy required to change the temperature of 1 kg of the substance by 1 °C.

a)

heat capacity

b)

specific heat capacity

c)

latent heat

d)

specific latent heat

42.

The unit of specific heat capacity is...

a)

$Jkg^{-1}$

b)

$JK^{-1}$

c)

$J\degree C^{-1}$

d)

$Jkg^{-1}K^{-1}$

43.

If water at $100\degree C$ is mixed with the SAME amount of water at $50\degree C$ the resulting mixture will have a temperature of

a)

$150\degree C$

b)

$100\degree C$

c)

$75\degree C$

d)

$50\degree C$

44.

If water at $90\degree C$ is mixed with TWICE the amount of water at $30\degree C$ the resulting mixture will have a temperature of

a)

$50\degree C$

b)

$60\degree C$

c)

$70\degree C$

d)

$120\degree C$

45.

The unit of specific latent heat is...

a)

$Jkg^{-1}$

b)

$JK^{-1}$

c)

$J\degree C^{-1}$

d)

$Jkg^{-1}K^{-1}$

46.

________________ is the amount of thermal energy required to change the state of 1 kg an object/substance at a constant temperature.

a)

heat capacity

b)

specific heat capacity

c)

latent heat

d)

specific latent heat

47.

Which will heat up faster?

a)

copper

b)

granite

c)

iron

d)

basalt

48.

Which will heat up slower?

a)

water

b)

lead

c)

granite

d)

iron

49.

Which of the following best explains why the sand at the beach is hotter than the water?

a)

Sand has a higher specific heat than water.

b)

Sand has a lower specific heat than water.

c)

There is more water than sand at the beach.

d)

There is more sand than water at the beach.

50.

Find the energy released by a copper block when it is cooled from 100^°C to 20^°C, given that the heat capacity of the block is 770 J^°C^-1.

a)

7.70x10⁴ J

b)

8.61x10⁴ J

c)

6.16x10⁴ J

d)

5.02x10⁴ J

51.

If an electric heater is supplied with an electric power of 2.0 kW to heat 4.0 kg of water for 1 minute, calculate the increase in temperature of the water. Assume that the specific heat capacity of water is 4200 J kg^-1 ⁰C^-1 and there is no energy loss to the surroundings.

a)

3.05⁰C

b)

7.1⁰C

c)

14⁰C

d)

30⁰C

52.

In order to make a cup of milk coffee at 78°C, 200 g of coffee is mixed up with 40 g of milk. If the original temperature of the coffee is 80°C, find the original temperature of the milk. Assume that there is no energy lost to the surroundings. Given that the specific heat capacity of coffee and milk are 4000 J kg^-1 °C^-1and 3900 J kg^-1 °C^-1 respectively.

a)

10.3°C

b)

20.7°C

c)

45.2°C

d)

67.7°C

53.

Given that the specific latent heat of fusion of a sample is 550 kJ kg^-1. Which of the following is correct?

a)

The mass of this sample is 1 kg.

b)

The energy needed to increase the temperature of 1 kg of this sample in solid state through 1^oC is 550 kJ.

c)

The energy needed to increase the temperature of 1 kg of this sample in liquid state through 1^oC is 550 kJ.

d)

The energy needed to change 1 kg of the material from solid state to liquid state is 550 kJ.

54.

Latent heat is

a)

the thermal energy absorbed or released at a boiling process during a change of phase

b)

the thermal energy absorbed or released at a constant temperature during a change of phase

c)

the thermal energy absorbed or released at a constant temperature during a change of phase of 1 kg object

d)

the thermal energy absorbed or released by an object to increase or decrease its temperature by 1 degree Celcius

55.

specific latent heat of vaporisation is

a)

the amount of energy required to change 1 kg of the substance from the solid to liquid phase without change in temperature

b)

the amount of energy required to change 1 kg of the substance from the liquid to gaseous phase without change in temperature

c)

the amount of energy required to change the temperature 1 kg of the substance by 1 degree Celcius

56.

What is the formula to calculate specific latent heat of vaporisation?

a)

L = Q/m

b)

c = Q/(mΔƟ)

c)

Q = mcΔƟ

d)

Q = mL

57.

Water molecules have the greatest kinetic energy... ?

a)

Ice at 0 ⁰C

b)

Water at 90 ⁰C

c)

Water at 373 K

d)

Steam at 150 ⁰C

58.

This is a diagram of ice. Ahmad measures the temperature of ice. After some time, he notices the ice melts. When the temperature of melting ice is measured, he found that _______________________________.

a)

The temperature is the same as the ice.

b)

The temperature is lower than the ice.

59.

The quantity of energy, Q that is absorbed or released during a change of phase of 1 kg of the substance without any change in its temperature.

This is the definition of

a)

Specific latent heat

b)

Latent heat

c)

Specific heat capacity

d)

Heat capacity

60.

Object A has a specific heat capacity of 4.45 J/g⁰C and object B has a specific heat capacity of 1.82 J/g⁰C.

Which object will heat up faster?

a)

Object A, it has a lower specific heat capacity.

b)

Object B, it has a lower specific heat capacity.

c)

Object A, it has a higher specific heat capacity.

d)

Object B, it has a higher specific heat capacity.

61.

Graphite has a specific heat capacity of 0.709 J/g⁰C. If a 20 gram piece of graphite is cooled from 38⁰C to 18⁰C, how much energy was lost by the graphite?

a)

283.6 J

b)

183.6 J

c)

203 J

d)

109 J

62.

What is the SI unit for temperature?

a)

Kelvin

b)

Celcius

c)

Fahrenheit

d)

All of these

63.

6200 J of energy is used to increase the temperature of a 1.2 kg metal block. The specific heat capacity of the metal block is 450 $J\ kg^{-1}\degree C^{-1}$ . What is the rise in temperature of the metal block ?

a)

9.6 $\degree$ C

b)

11.5 $\degree$ C

c)

15.0 $\degree$ C

d)

360.0 $\degree$ C

64.

The temperature of a 6.0 g sample of glass changed from 20.0°C to 45.0°C when it absorbed 550 J of thermal energy. What is the specific heat capacity of this glass?

a)

0.27 J/g °C

b)

3.7 J/g °C

c)

130 J/g °C

d)

12 J/g °C

65.

The specific heat of platinum is 0.133 J/g°C. How much energy(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

66.

What is specific heat capacity?

a)

The power needed to raise the temperature of 1 kg of a substance by 1^oC.

b)

The energy needed to raise the temperature of 1 kg of a substance by 1^oC.

c)

The temperature increase of 1 kg of a substance when it is heated for 1 minute.

d)

The mass of a substance whose temperature will increase by 1^oC when heated for 1 minute.

67.

Water has specific heat capacity of 4180 J/kg^oC and Lead has specific heat capacity 128 J/kg^oC. Assume 1 kg of water and 1 kg of Lead are at 50^oC. Which material would take longer to cool down to room temperature?

a)

Water

b)

Lead

c)

Both would cool down at same rate

d)

Impossible to tell

68.

A high specific heat capacity means...

a)

It heats up quickly with energy added

b)

It requires more energy to change temperature

69.

A pot of water is boiled from 20 °C to 100 °C. What is the ΔT ?

a)

20 °C

b)

100 °C

c)

40 °C

d)

80 °C

70.

How much energy is needed to raise the temperature of 10.0 g of aluminum from 22 °C to 55 °C, if the specific heat of aluminum is 0.90 J/g°C

a)

297 J

b)

450 J

c)

698 J

d)

802 J

Reset

Similar Resources on Wayground

67 questions

Physics Ch 4 Forces & the Laws of Motion

Worksheet

•

11th - 12th Grade

65 questions

Work, Power, and Energy Review

Worksheet

•

11th Grade

73 questions

Newton's Laws and Applications

Worksheet

•

9th - 12th Grade

67 questions

Chapter 15: Electrostatic

Worksheet

•

12th Grade - University

69 questions

Properties of Matter

Worksheet

•

5th Grade - University

65 questions

Ramp & Marble Lab Review

Worksheet

•

9th - 12th Grade

71 questions

Direct Current DP024

Worksheet

•

9th - 12th Grade

70 questions

Con. E 1 Review

Worksheet

•

8th - 11th Grade