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Liquid & Solids Review

Total questions: 66

Worksheet time: 1hrs 5mins

Name
Class
Date
1.

What phase change occurs with the addition of heat to a substance.

a)

Freezing

b)

Evaporation

c)

Melting

d)

Condensation

2.

Phase change going from a Solid to a Gas...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Recombination

3.

Phase change going from a Gas to a Solid...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Vaporization

4.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

5.

Are the particles moving faster or slower as time goes on?

a)

Faster

b)

Slower

6.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

7.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

8.

What state of matter is pictured?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

9.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
10.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
11.
Molecules are closest together in a 
a)
Solid
b)
Liquid
c)
Gas
12.
In a solid, the particles
a)
vibrate in place
b)
slide past one another
c)
overcome the strong attraction
13.

A phase change is a chemical or physical change?

a)

Physical

b)

Chemical

14.

When an object undergoes phase change, its mass

a)

increases

b)

stays the same

c)

decreases

15.
Water exists as a _____________ at 3 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
16.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
17.
What phase change(s) may occur at pressures below 4.58 mmHg?
a)
sublimation/deposition
b)
melting/freezing
c)
all phase changes are possible at these pressures
d)
vaporization/condensation
18.
The pressure is increased on a sample of water at 0 °C from 0 mmHg to 800 mmHg.  In order, what changes occur?
a)
deposition, melting
b)
sublimation, melting
c)
condensation, freezing
d)
deposition, freezing
19.
Based on this phase diagram, which state is the most dense?
a)
gas
b)
solid
c)
liquid
d)
solid and liquid have equal densities
20.
Water will boil at temperatures above 100 °C at pressures __________ 760 mmHg.
a)
below
b)
above
c)
equal to
d)
significantly below
21.
Which statement is true for carbon dioxide at -60 °C?
a)
All three phases are possible.
b)
It can exist as a solid or a gas, depending on pressure.
c)
It is a solid.
d)
With enough pressure it can be melted.
22.
Based on its phase diagram, which is the most dense state for CO2?
a)
gas
b)
liquid
c)
solid
d)
supercritical fluid
23.
What is true regarding CO2 for temperatures above 31 °C?
a)
It can never be liquified.
b)
It decomposes.
c)
It has a high pressure.
d)
It is a plasma.
24.
At 10 atm, dry ice is heated from -100 °C to 30 °C.  What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
25.
What is the normal melting point of CO2?
a)
-78.5 °C
b)
-56.7 °C
c)
31 °C
d)
It doesn't have a normal melting point.
26.
What is the normal boiling point of CO2?
a)
-78.5 °C
b)
-56.7 °C
c)
31 °C
d)
It doesn't have a normal boiling point.
27.
Water exists as a _____________ at 3 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
28.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
29.
What phase change(s) may occur at pressures below 4.58 mmHg?
a)
sublimation/deposition
b)
melting/freezing
c)
all phase changes are possible at these pressures
d)
vaporization/condensation
30.
The pressure is increased on a sample of water at 0 °C from 0 mmHg to 800 mmHg.  In order, what changes occur?
a)
deposition, melting
b)
sublimation, melting
c)
condensation, freezing
d)
deposition, freezing
31.
Based on this phase diagram, which state is the most dense?
a)
gas
b)
solid
c)
liquid
d)
solid and liquid have equal densities
32.
Water will boil at temperatures above 100 °C at pressures __________ 760 mmHg.
a)
below
b)
above
c)
equal to
d)
significantly below
33.
Which statement is true for carbon dioxide at -60 °C?
a)
All three phases are possible.
b)
It can exist as a solid or a gas, depending on pressure.
c)
It is a solid.
d)
With enough pressure it can be melted.
34.
Based on its phase diagram, which is the most dense state for CO2?
a)
gas
b)
liquid
c)
solid
d)
supercritical fluid
35.
What is true regarding CO2 for temperatures above 31 °C?
a)
It can never be liquified.
b)
It decomposes.
c)
It has a high pressure.
d)
It is a plasma.
36.
At 10 atm, dry ice is heated from -100 °C to 30 °C.  What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
37.
What is the normal melting point of CO2?
a)
-78.5 °C
b)
-56.7 °C
c)
31 °C
d)
It doesn't have a normal melting point.
38.
What is the normal boiling point of CO2?
a)
-78.5 °C
b)
-56.7 °C
c)
31 °C
d)
It doesn't have a normal boiling point.
39.
What state of matter is X?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
40.
What state of matter is Y?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
41.
What state of matter is Z?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
42.
What change occurs from F to E?
a)
sublimation
b)
deposition
c)
melting
d)
condensation
43.
What change occurs from E to C?
a)
sublimation
b)
freezing
c)
melting
d)
boiling
44.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
45.
What is the normal boiling point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
46.
What is the normal melting point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
47.
What is point A?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
48.
What is point B?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
49.
Above the temperature of point B, this substance exists as a ____________.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
50.
Below the temperature of point B, this substance can exist as a ____________.
a)
solid only
b)
liquid only
c)
gas only
d)
either a solid, liquid or gas
51.
At 0.10 atm, what phase(s) can exist?
a)
solid, liquid or gas
b)
liquid or gas
c)
solid only
d)
gas only
52.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
53.
Does HCl have hydrogen bonding?
a)
yes
b)
no
54.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

55.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

56.
As pressure decreases, boiling point___
a)
decreases
b)
increases
c)
decreases then increases
d)
increases then decreases
57.
Liquids with weak intermolecular forces
a)
contain a lot of kinetic energy
b)
easily evaporate
c)
cannot diffuse
d)
freeze easily
58.
water have a low vapor pressure because
a)
it has strong london dispersion forces acting between its molecules
b)
it has strong hydrogen bonds acting between its molecules
c)
it has a weaker force of attraction between its molecules
d)
it is very volatile
59.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

60.

Which liquid has the highest vapor pressure at 75oC?

a)

ethanoic acid

b)

ethanol

c)

propanone

d)

water

61.

At which temperature is the vapor pressure of ethanol equal to the vapor pressure of propanone at 35oC?

a)

35oC

b)

60oC

c)

82oC

d)

95oC

62.

Which model represents a HIGHER vapor pressure?

a)

A

b)

B

63.

Which particle level model represents the pure substance with STRONGER intermolecular attractions?

a)

A

b)

B

64.

What is vapor pressure?

a)

the force of the gas above a liquid

b)

the force of a gas below a liquid

c)

the force of a liquid below a gas

d)

boiling point

e)

evaporation

65.

Why do sealed jars with liquid in them reach equilibrium?

a)

evaporation rates equal condensation rates

b)

all the liquid evaporates

c)

all the liquid condenses

d)

there is an equal amount of liquid and gas

e)

they do no not reach equilibrium

66.

Do unsealed jars with liquid in them reach equilibrium?

a)

evaporation rates equal condensation rates

b)

all the liquid evaporates

c)

all the liquid condenses

d)

there is an equal amount of liquid and gas

e)

they do no not reach equilibrium

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