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States of Matter and Heat Flow

Total questions: 128

Worksheet time: 2hrs 27mins

Name
Class
Date
1.
Heat transfer always goes from-
a)
Cold to Hot
b)
Hot to Cold
c)
Heat doesn't transfer
d)
Freezing to Cold
2.
What is heat?
a)
How fast something warms up.
b)

The measure of the average kinetic energy of all the particles in an object.
c)

The transfer of energy from one object to another because of a temperature difference.
d)
The amount of kinetic energy in a substances
3.
The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius is ________
a)
Heat energy
b)
Specific heat
c)
convection
d)
thermal energy
4.
When ice melts, its temperature ________. 
a)
decreases
b)
increases
c)
remains the same
5.

Heat is the transfer of _______ between substances of different temperatures

a)

Energy

b)

Atoms

c)

Molecules

6.

A material that transfers heat energy easily

a)

Conductor

b)

Radiator

c)

Insulator

7.
A liquid is
a)
a substance that does not have a definite shape or volume
b)
a substance with a definite volume, but no definite shape
c)
a substance with a definite shape and volume
d)
a substance whose particles vibrate
8.
A solid is
a)
a substance that does not have a definite shape or volume
b)
a substance with a definite volume, but no definite shape
c)
a substance with a definite shape and volume
d)
a substance whose particles glide past one another
9.
Which states of matter have a definite volume?
a)
solid and gas
b)
solid and liquid
c)
gas and liquid
d)
solid, liquid, and gas
10.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
11.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
12.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

13.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

14.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
15.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
16.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
17.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
18.
In an exothermic process, the surroundings are gaining energy.
a)
True
b)
False
19.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
20.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

21.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
22.
Specific heat of water is  4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more heat energy to raise the temperature?
a)
Water
b)
Wood
c)
Both are same
23.
What does "ΔH" mean? 
a)
A change in health
b)
A change in heat
c)
A change in height
d)
A change in temperature
24.
Water molecules have the greatest kinetic energy in
________________
a)
Ice at 0 °C.
b)
Water at 373 K.
c)
Water at 98 °C
d)
Steam at 150 °C.
25.
How many Joules of energy are required to change 10 gram of ice at -2 οC to water at 20 οC?
a)
440 J
b)
880 J
c)
3,840 J
d)
66,000 J
26.
How many Joules of energy are required to make 100 grams of ice at 0 οC completely melt?
a)
200 J
b)
400 J
c)
30,000 J
d)
2,000,000 J
27.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
28.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C? (show your work)

a)

-80,256

b)

80.256

c)

80,256

d)

-80.256

29.

Energy of being in motion

a)

Calorie

b)

calorimetry

c)

exothermic

d)

kinetic energy

30.

Match Definition to Term:

Heat of Fusion

a)

The difference in energy between the solid and liquid states for a given amount of substance

b)

The difference in energy between the liquid and gas states for a given amount of substance

c)

The energy associated for a 1 degree temperature change for a given amount of a substance

31.

Match Definition to Term:

Specific Heat

a)

The difference in energy between the solid and liquid states for a given amount of substance

b)

The difference in energy between the liquid and gas states for a given amount of substance

c)

The energy associated for a 1 degree temperature change for a given amount of a substance

32.

Match Definition to Term:

Heat of Vaporization

a)

The difference in energy between the solid and liquid states for a given amount of substance

b)

The difference in energy between the liquid and gas states for a given amount of substance

c)

The energy associated for a 1 degree temperature change for a given amount of a substance

33.

For Water Hf = 6.01 kJ mol-1 and Hv = 40.14 kJ mol-1. Find the energy change associated with boiling 10g of water.

a)

22.3 kJ

b)

401 kJ

c)

60.1 kJ

d)

3.34 kJ

34.

A 100 g sample of a metal was heated to 100oC and then quickly transferred to an insulated container holding 100 g of water at 22oC. The temperature of the water rose to reach a final temperature of 35oC. Choose all that are true.

a)

The metal lost more energy than the water gainer

b)

The amount of energy lost by the metal is equal to the energy gained by the water

c)

The metal must have a higher specific heat than the water

d)

The water must have a higher specific heat than the metal

35.
Which is a quality that only gasses display
a)
Spread out to fill all available space
b)
Take the shape of their container
c)
Can't be compressed
d)
All of these
36.
Pressure is caused by ______.
a)
gravity.
b)
gas molecules colliding with each other.
c)
gas molecules colliding with surfaces of the container.
d)
gas molecules reacting with each other.
37.
What happens to the average kinetic energy of matter when it is heated?
a)
It increases
b)
It decreases 
c)
It doesn't change
d)
It cannot be determined
38.
In a solid, the particles
a)
vibrate in place
b)
slide past one another
c)
overcome the strong attraction
39.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
40.
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.
41.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
42.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
43.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
44.

All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London Dispersion forces. Which of these has ONLY London forces?

a)

I2

b)

NH3

c)

OCl2

d)

SH2

45.

What is the primary intermolecular force in liquid acetone (pictured here)?

a)

Dispersion forces

b)

Dipole dipole forces

c)

Hydrogen bonds

d)

Covalent Bonds

46.

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

47.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
48.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
49.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
50.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
51.

Which substance would have the highest boiling point at standard pressure?

a)

H2O

b)

CCl4

c)

CO2

d)

NBr3

52.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

53.

The forces that hold the atoms in a CCl4 molecule together are _______, and the forces that hold the molecules together in sample are _________.

a)

intermolecular (covalent); intramolecular (dipole-dipole)

b)

intermolecular (dipole-dipole); intramolecular (dipole-dipole)

c)

intramolecular (covalent); intermolecular (London Dispersion)

d)

intramolecular (covalent); intermolecular (dipole-dipole)

54.
Will this molecule be polar or nonpolar? CH4
a)
polar
b)
nonpolar
55.
Is hydrogen bonding or london dispersion forces a stronger force?
a)
London Dispersion Forces
b)
Hydrogen Bonding
56.
Define volatility
a)
the tendency of a substance to increase in speed
b)
The tendency of a substance to solidify
c)
The tendency of a substance to condense
d)
The tendency of a substance to vaporize
57.
What kind of relationship does boiling point and vapor pressure have?
a)
Direct
b)
Inverse
58.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
59.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
60.
CO2 has polar bonds but is a NON POLAR molecule. Why?
a)
it has an asymmetrical shape
b)
bond polarity between C and O atoms cancel
c)
net dipole moment exist between atoms in molecule
d)
bond polarity exist between C+ and O-
61.

Dipole - dipole attractions are attractions between the - end of one polar molecule and the + end of another polar molecule.

a)

True

b)

False

62.
Both _____ _____ and _____ _____ rely upon the strength of interparticular attraction between the liquid particles. 
a)
surface tension; capillary action 
b)
covalent bonds; hydrogen bonds
c)
sodium ions; water molecules
63.
The _____ the intermolecular forces, the more molecules will enter the vapor phase. 
a)
stronger
b)
weaker
c)
sturdier 
d)
polar
64.
2. A change of state from a liquid to a solid is called....
a)
Melting
b)
Freezing
c)
Evaporation
65.
7. All phase changes (changing states) requires energy to be added or taken away.
a)
True
b)
False
66.
change from liquid to gas is called....
a)
expansion
b)
evaporation
c)
condensation
d)
sublimation
67.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
68.
During a phase change which type of energy is most likely to increase?
a)
Kinetic 
b)
Potential 
c)
Solar
d)
electrical 
69.
What line segment represents only the solid state?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
70.
Which process takes the longest to occur?
a)
melting
b)
boiling
c)
freezing
d)
heating the solid
71.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
72.
Between which points is the substance changing state?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
73.
The graph shows a cooling curve for an unknown substance.  What is happening during segment DE?
a)
boiling
b)
condensation
c)
freezing
d)
melting
74.
True or false: melting and freezing occur at the same temperature.
a)
True
b)
False
75.

This force is sometimes called an induced dipole-induced dipole attraction.

a)

Debye (Induced) Dipole

b)

(London) Dispersion Forces

c)

Hydrogen "Bonds"

d)

Dipole-Dipole

76.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
77.

Which type of solid has strong covalent bonds, only, that hold the crystal together in the solid phase?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Network

78.

Which is NOT an intramolecular force?

a)

Polar Covalent Bond

b)

Nonpolar Covalent Bond

c)

London Dispersion Force

d)

Ionic Bond

79.

Which has the weakest forces between particles (usually)?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

80.

Which structure consists of a giant lattice of cations and anions held together by strong electrostatic forces of attraction?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

81.

Which structure consists of a giant lattice of regularly arranged cations surrounded by a sea of delocalized electrons.

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

82.

Which of the following types of bonding results in materials which are usually solids at room temperature?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

83.

Which of the following types of bonding results in materials which are usually liquid or gases at room temperature?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

84.

Which of the following types of bonding results in materials which have the lowest melting and boiling points?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

85.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
86.

Forces of attraction or repulsion that act within a molecule

a)

Conductivity

b)

Thermal

c)

Intermolecular

d)

Intramolecular

87.

The temperature of a substance that occurs when the vapor pressure of the liquid is equal to the pressure above the surface of the liquid.

a)

Melting Point

b)

Evaporation

c)

Boiling Point

d)

Freezing Point

88.

Forces of attraction or repulsion that act between neighboring particles

a)

Polar

b)

Intermolecular

c)

Intramolecular

d)

Thermal

89.

Describes a molecule in which one or more atoms is slightly negative and one or more is slightly positive

a)

Nonpolar

b)

Polar

c)

Bond

90.

The pressure exerted by a vapor over a liquid

a)

Melting point

b)

Boiling point

c)

Evaporation

d)

Vapor Pressure

91.
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
92.
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.
93.
What state of matter is Y?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
94.
What state of matter is Z?
a)
solid 
b)
liquid
c)
gas
d)
supercritical fluid
95.
What change occurs from E to C?
a)
sublimation
b)
freezing
c)
melting
d)
boiling
96.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
97.
What is the normal boiling point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
98.
What is the normal melting point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
99.
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
100.
At 0.10 atm, what phase(s) can exist?
a)
solid, liquid or gas
b)
liquid or gas
c)
solid only
d)
gas only
101.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
102.
What is point A?
a)
triple point
b)
critical point
c)
equilibrium point
d)
normal melting point
103.

As you increase pressure on water, what happens to the melting point and boiling point?

a)

They both increase

b)

The melting point increases, but the boiling point decreases.

c)

The melting point decreases, but the boiling point increases

d)

They both decrease

104.

The boiling point of water on Mount Everest would be_________.

a)

Less than normal

b)

More than normal

c)

The same as normal

105.

The boiling point of water in a pressure cooker would be_________.

a)

Less than normal

b)

More than normal

c)

The same as normal

106.
The strength of intermolecular forces varies between liquids, therefore they will have
a)
different equilibrium vapor pressure
b)
the same equilibrium vapor pressure
c)
different temperatures
d)
the same amount of kinetic energy
107.
During a phase change, the temperature
a)
increases
b)
decreases
c)
fluctuates
d)
stays the same
108.
In order to turn liquid water into water vapor, you must:
a)
add chemicals
b)
increase the pressure on it
c)
add energy
d)
take away energy
109.
Above the temperature of point B, this substance exists as a ____________.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
110.
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
111.
When the atmospheric pressure equals the equilibrium vapor pressure ___ occurs.
a)
freezing
b)
melting
c)
boiling
d)
sublimation
112.
Liquids with weak intermolecular forces
a)
contain a lot of kinetic energy
b)
easily evaporate
c)
cannot diffuse
d)
freeze easily
113.
when a liquid becomes vapor, its gas particles begin to exert...
a)
air pressure
b)
vapor pressure
c)
equilibrium pressure
d)
no pressure
114.
why does a gas with a lower vapor pressure have a higher boiling point
a)
its molecules need more energy in order to break free from strong attraction
b)
there are strong forces of attraction between its particles
c)
it has a lower volatility
d)
all of the answer
115.
How do gas molecules move?
a)
In an orderly fashion
b)
Constantly and randomly
c)
In straight-line paths
d)
In a circular motion
116.
The average kinetic energy of all the molecules in liquid water at 80⁰ C is the same as the average kinetic energy of the molecules in oxygen gas at 80⁰
a)
True
b)
False
117.

Why is the boiling point in in the mountains less than 100 degrees?

a)

Because there are more minerals in the water.

b)

Because water always boils at 100 degrees Celsius.

c)

Because there is less atmospheric pressure in the mountains.

d)

Because our water is cleaner in the mountains.

e)

Because there is more atmospheric pressure in the mountains.

118.

Liquids with low volatility tend to have

a)

weak intermolecular forces

b)

high vapor pressure

c)

low vapor pressure

d)

strong intermolecular forces

e)

high boiling points

119.

Liquids with weak intermolecular forces tend to have

a)

low boiling points

b)

high vapor pressure

c)

high volatility

d)

low vapor pressure

e)

low volatility

120.

substance that does not contain water

a)

anhydrous

b)

desiccant

c)

hygroscopic

d)

deliquescent

121.

compound that contains water of hydration

a)

water of hydration

b)

hygroscopic

c)

hydrate

d)

anhydrous

122.

When a hydrate loses its water of hydration

a)

dissolution

b)

condensation

c)

effloresce

d)

dessicate

123.

compounds that remove moisture from air

a)

hygroscopic

b)

solute

c)

solvent

d)

colloid

124.

substance used to absorb moisture from the air and create a dry atmosphere

a)

desiccant

b)

solvent

c)

suspension

d)

oil

125.

substances that remove sufficient water from the air to dissolve completely and form solutions

a)

suspension

b)

colloid

c)

None of these

d)

deliquescent

126.
When a hydrate loses its water of hydration, it is said to ________.
a)
Dehydrate
b)
Effloresce
c)
Gain surface tension
d)
Lose surface tension
127.

A solid having randomly arranged atoms or molecules is called __________________.

a)

Amorphous

b)

Ductility

c)

Crystalline

d)

Strength

128.

A(n) _______________solid has an orderly, repeating arrangement of particles.

a)

Hardness

b)

Malleability

c)

Strength

d)

Crystalline

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