A
What is the process called when a solid turns directly into a gas?
A. Condensation
B. Sublimation
C. Freezing
D. Melting
B. Sublimation
True or False: Condensation is the change of a gas to a liquid
True
What phase change occurs when water changes from liquid to solid?
Freezing
Which phase change releases energy?
A. Melting
B. Boiling
C. Condensation
D. Freezing
D. Freezing
When a gas turns into a solid without becoming a liquid, it is called __________.
Deposition
What happens to the kinetic energy of particles during melting?
A. It decreases as particles lose energy and move less
B. It remains constant with no energy change at all
C. It increases as particles gain energy and break free
D. It disappears completely when melting takes place
C. It increases as particles gain energy and break free
Which of the following best describes the particles in a solid?
A. Freely moving and far apart
B. Vibrating in fixed positions
C. Random and fast-moving
D. Sliding over each other
B. Vibrating in fixed positions
True or False: Solids can be compressed easily due to the spacious orientation between particles.
False
What determines how fast particles move in a substance?
A. The container size
B. The temperature
C. The shape of particles
D. The color of the substance
B. The temperature
Which of the following has a definite shape and definite volume?
A. Liquid
B. Solid
C. Gas
D. Plasma
B. Solid
During melting, heat is being __________ by the substance.
absorbed
What is the heat of fusion?
A. Heat required to boil a liquid
B. Heat required to freeze a gas
C. Heat required to melt a solid
D. Heat required to condense a vapor
C. Heat required to melt a solid
What do you call the phase change where plasma turns into gas?
Recombination
True or False: Latent heat causes a change in temperature during a phase change.
False
What happens during boiling in terms of energy?
A. Heat is released to form vapor
B. Heat's absorbed to overcome intermolecular forces
C. No energy change occurs during boiling
D. Heat is absorbed to decrease molecular motion
B. Heat is absorbed to overcome intermolecular forces
A 200 g metal heats up from 25°C to 75°C using 8000 J. What is its specific heat?
c=0.8 J/g°C
How much heat is required to melt 150 grams of ice at 0°C?
(Heat of fusion of ice = 334 J/g)
Q=50,100 joules
The heat of fusion of ice is 334 J/g. If 16,700 joules of heat is used to melt a block of ice, what is its mass?
m=50 grams
A 200 g sample of copper absorbs 3,600 J of heat. If the specific heat of copper is 0.39 J/g°C, what is the change in temperature of the copper?
∆T=46.15°C
A substance absorbs 4,500 J of heat and its temperature rises by 30°C. If its specific heat is 0.50 J/g°C, what is its mass?
m=300 grams
The Heat of fusion of ice is 334 J/g. If a 0.5 kg block of ice is to be melted at 0°C, how much energy is needed to melt it completely?
Q=167,000 Joules
A 75,000 mg sample of a liquid absorbs 165,000 J of heat to vaporize completely. What is its heat of vaporization?
Q=2,200 J/g
A substance absorbs 2,400 J of heat and its temperature increases by 30°C. If the specific heat is 0.40 J/g°C, what is the mass in milligrams?
m=200,000 milligrams
A 1.2 kg sample absorbs 10,800 J of heat and its temperature rises from 20°C to 60°C. What is the specific heat capacity of the material?
c=0.23 J/g°C
A 0.227 kg sample absorbs 5,670 J of energy. If its temperature change is from 68°F to 45°C. What would be the specific heat of the sample?
c=1.01 J/g°C