Free Printable Module 6 Review

1.

The energy of movement is ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

2.

The more energy that particles have, the ___ they move.

a)

slower

b)

faster

3.

The force of attraction between molecules is ___.

a)

intermolecular forces

b)

bridge forces

c)

chemical bonds

4.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

5.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

6.

These properties describe a ___.

a)

solid

b)

liquid

c)

gas

7.

Collisions in which particles transfer all their kinetic energy to other particles are called ___.

a)

elastic

b)

inelastic

8.

Which one of these is NOT an Ideal Gas Assumption?

a)

Gas particles are hard, round spheres.

b)

Gas particles are strongly attracted to one another.

c)

Gas particles do not take up space.

d)

Gas particles collide perfectly elastically.

9.

What is the first assumption of the Kinetic Theory of Matter?

a)

Matter consists of molecules and atoms

b)

Gases are the same in all matter

c)

Matter is the same as kinetic energy

10.

Which is not a phase of matter?

a)

Solid

b)

Liquid

c)

Plasma

d)

Gas

e)

Nuclear

11.

Which of the physical states of water contains particles with the lowest kinetic energy?

a)

Water

b)

Ice

c)

Steam

d)

Melting ice

12.

_______ is an explanation of how particles in matter behave

a)

Boyle's Law

b)

Charles' Law

c)

Kinetic Molecular Theory

13.

Temperature is a direct measure of:

a)

The density of the particles within a substance.

b)

The average speed of the particles within a substance.

c)

How often the particles collide with the walls of their container.

14.

As the temperature of a substance increases:

a)

The speed, and average kinetic energy of the particles, both increase.

b)

The speed, and average kinetic energy of the particles, both decrease.

c)

The speed of the particles increases, but the average kinetic energy of the particles decreases.

d)

The speed of the particles decreases, but the average kinetic energy of the particles increases.

15.

Absolute Zero is defined as:

a)

The lowest temperature which can be achieved by scientists.

b)

The lowest temperature which can be recorded on a thermometer.

c)

The theoretical temperature at which all particles stop moving.

d)

The temperature of a cold block of copper.

16.

True or false: melting and freezing occur at the same temperature!

a)

True

b)

False

c)

I don't know

17.

Gas 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.

18.

Between which two points is the solid cooling?

a)

A <---- B

b)

B <----> C

c)

C <---- D

d)

D <----> E

e)

E <---- F

19.

Between which two points is the gas heating up?

a)

A ----> B

b)

B <---- C

c)

C ----> D

d)

D ----> E

e)

E ----> F

20.

Between which two points is the gas condensing?

a)

A <---- B

b)

B <---- C

c)

C <---- D

d)

D <---- E

e)

E <---- F

21.

Between which points is the temperature of the substance remaining constant?

a)

A-B only.

b)

A-B, C-D, E-F

c)

B-C only.

d)

B-C, D-E

22.

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

23.

The graph shows a cooling curve for an unknown substance. What is happening during segment DE?

a)

boiling

b)

condensation

c)

freezing

d)

melting

24.

In which segment is the kinetic energy remaining constant?

a)

A-B

b)

B-C

c)

C-D

d)

E-F

25.

This curve indicates what about the heat energy?

a)

heat energy is being added or absorbed

b)

heat energy is being removed

26.

What is happening to the particles in the substance between points A and B?

a)

Melting

b)

Freezing

c)

Speeding Up

d)

Slowing Down

27.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

28.

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

29.

7. All phase changes (changing states) requires energy to be added or taken away.

a)

True

b)

False

30.

All changes in the state of matter of a substance requires

a)

vibration

b)

water

c)

permission

d)

energy

31.

During a phase change what happens to temperature?

a)

it increases

b)

it decreases

c)

depends; if being heated it increases, if being cooled it decreases

d)

stays constant

32.

When molecules move slower, kinetic energy

a)

increases

b)

stays the same

c)

decreases

d)

none of these

33.

Which of these explain how a natural phenomenon works or happens?

a)

theory

b)

law

34.

Which of these describes a natural phenomenon or relationship that always occurs under specific conditions

a)

theory

b)

law

35.

If a gas has constant temperature and number of moles and its Pressure goes up, what happens to its volume?

a)

It goes up

b)

It goes down

c)

It stays the same

36.

If a gas has constant volume and number of moles and its temperature goes up, what happens to its pressure?

a)

It goes up

b)

It goes down

c)

It stays the same

37.

If a gas has constant pressure and number of moles and its temperature goes down, what happens to its volume?

a)

It goes up

b)

It goes down

c)

It stays the same

38.

If a gas has constant temperature and pressure and its number of moles goes up, what happens to its volume?

a)

It goes up

b)

It goes down

c)

It stays the same

39.

What is the correct formula for Boyle's Law?

a)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

b)

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

c)

$P_1V_1=P_2V_2$

d)

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

40.

What is the correct formula for Charles's Law?

a)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

b)

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

c)

$P_1V_1=P_2V_2$

d)

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

41.

What is the correct formula for Gay-Lussac's Law?

a)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

b)

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

c)

$P_1V_1=P_2V_2$

d)

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

42.

What is the correct formula for Avogadro's Law?

a)

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

b)

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

c)

$P_1V_1=P_2V_2$

d)

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

43.

1. A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kPa pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters?

a)

219 KPa

b)

222 KPa

c)

567 KPa

d)

654 KPa

44.

A sample of hydrogen at 1.5 atm had its pressure decreased to 0.50 atm producing a new volume of 750 mL. What was its original volume?

a)

245 ml

b)

345 ml

c)

123 ml

d)

250.mL

45.

Edelman and Gronkowski want to play a game of beach volleyball. If the beach ball has a volume of 261 L at a temperature of 502 K, what will the temperature of the balloon be if the volume decreases to 176 L?

a)

744 K

b)

0.0030 K

c)

339 K

d)

512 K

46.

If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be

a)

250 mL

b)

204 mL

c)

196 mL

d)

160 mL

47.

Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 ˚C to 30.0 ˚C.

a)

.75 atm

b)

.93 atm

c)

1.03 atm

d)

2.96 atm

48.

A gas thermometer measures temperature by measuring the pressure of a gas inside the fixed volume container. A thermometer reads a pressure of 248 kPa at 0˚C. What is the temperature when the thermometer reads a pressure of 345 kPa?

a)

380 K

b)

420 K

c)

460 K

d)

580 K

49.

If 3.25 mol of Ar occupies 100. L at a particular temp and pressure, what volume does 14.15 mol of Ar occupy under same condition?

a)

435 L

b)

225 L

c)

100 L

d)

522 L

50.

A 2.00 L sample of pure oxygen gas (O₂) is measured at STP. How many moles of oxygen is this?

a)

24.4 mol

b)

0.007 mol

c)

1.44 mol

d)

0.09 mol

51.

How many moles of argon gas are present in 18.83 liters?

a)

4.22 mols

b)

421.79 mols

c)

0.84 mols

d)

0.79 mols

52.

Determine the volume, in liters, occupied by 42 mols of oxygen gas.

a)

944 L

b)

940.8 L

c)

0.420 L

d)

1.875 L

53.

At room temperature and pressure condition, How many liters of NH₃ are needed to react completely with 30.0L of NO?

4NH₃+6NO --> 5N₂ + 6H₂O

a)

5.0 L

b)

20.0 L

c)

7.5 L

d)

120.0 L

54.

2CO (g) + O_{2 (g)}--> 2CO₂ (g)

How many liters of carbon dioxide (CO₂) are produced from 10L of carbon monoxide (CO)?

a)

10

b)

20

c)

1

d)

5

55.

Determine the amount of moles of BaCl₂ that are in 436 g of the compound.

a)

3.5 mol

b)

2.1 mol

c)

4.6 mol

d)

2.7 mol

56.

Determine the amount of moles in CuBr that are in 276.9 g of the compound.

a)

3.2 mol

b)

1.7 mol

c)

2.1 mol

d)

1.9 mol

57.

What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT

a)

14.19 atm

b)

16.53 atm

c)

18.42 atm

d)

22.54 atm

58.

Gases have...

a)

A definite shape and volume

b)

A definite shape but no definite volume

c)

No definite shape but a definite volume

d)

No definite shape or volume

59.

A 7.50 liter sealed jar at 18 °C contains 0.125 moles of oxygen and 0.125 moles of nitrogen gas. What is the pressure in the container?

a)

7.38 atm

b)

0.796 atm

c)

0.684 atm

d)

0.398 atm

60.

When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pressure of 700 mm Hg. What is the volume of the container?

a)

0.557 Liters

b)

6.57 Liters

c)

8.74 Liters

d)

0.0087 Liters

Module 6 Review

Total questions: 60

Worksheet time: 2hrs 30mins

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