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Gas Laws

Total questions: 102

Worksheet time: 4hrs 36mins

Name
Class
Date
1.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
2.
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
3.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
4.
In Charles' Law the pressure remains constant.
a)
True
b)
False
5.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
6.
True or False: Gases can be compressed. 
a)
True
b)
False
7.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
8.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
9.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
10.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
11.
What causes pressure?
a)
The walls of the container
b)
The vacuum in the container
c)
The collisions of the particles
d)
Atmospheric pressure acting on the outside walls
12.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
13.
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
14.
A gas of volume V is placed in a balloon.  Determine the new volume of the balloon if the pressure is tripled. The new volume will be ____ what it was originally.  
a)
1/3 of
b)
1/6 of
c)
1/9 of
d)
 9 times
15.
A gas of volume V is placed in a balloon. The absolute (Kelvin) temperature is tripled. The volume will be _____ what it was originally. 
a)
1/3
b)
1/6
c)
3 times
d)
6 times
16.
Boyle's law shows the volume and pressure of a gas are always ........
a)
inversely proportional 
b)
directly proportional 
17.
Charles's law shows that the temperature and volume of a gas are always........
a)
inversely proportional 
b)
directly proportional 
18.
Temperature describes  the ______________ of particles.
a)
volume
b)
mass
c)
motion
d)
conductivity
19.
The word inverse means.......
a)
the same
b)
opposite 
20.
When a basketball is left outside in the cold it goes flat because the volume of air inside the ball has been reduced. What  gas law does this represent?
a)
Boyle's Law
b)
Charles's Law
21.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
22.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
23.
A gas at 928 kpa, 129 C occupies a volume of 569 L. Calculate the volume at 319 kpa and 32 C.
a)
410.61 L
b)
418.18 L
c)
1100 L
d)
1400 L
24.
If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?
a)
1.75 atm
b)
1.8 atm
c)
1.3 atm
d)
1.29 atm
25.
Gas Laws involve what three terms?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
26.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
27.
Whose law states that as pressure goes up, volume goes down?
a)
Charles 
b)
Boyle
c)
Aglow
d)
Mazias 
28.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
29.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

30.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.1 atm

c)

1.6 atm

d)

3.4 atm

31.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

32.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

33.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

34.
Gas Laws involve what three terms?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
35.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
36.
If the pressure exerted by a gas at 298 K in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
P1/T1 = P2/T2
b)
PV = nRT
c)
V1/n1 = V2/n2
d)
P1V1 = P2V2
37.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
38.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
39.
100 degrees Celsius is equal to _______ Kelvin. 
a)
0 K
b)
273 K
c)
173 K
d)
373 K
40.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
41.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
42.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K
43.

What is the pressure of a car tire that had an initial pressure of 1.8 atm but was heated from 38°C to 123°C?

a)

0.9 atm

b)

2.4 atm

c)

1.6 atm

d)

3.4 atm

44.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
45.

A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?

a)

60.0 mL

b)

15.0 mL

c)

27.5 mL

d)

32.5 mL

46.

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

a)

3670 atm

b)

0.245 atm

c)

4.08 atm

d)

605 atm

47.
What will happen to the volume of a gas under constant temperature if the pressure increases?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
48.
f a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?
a)
9 L
b)
.69 L
c)
1.44 L
49.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
50.
1. If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?
a)
1.5L
b)
45 L
c)
1.44L
d)
27.4L
51.

What is the temperature of 3.45 moles of a gas at a pressure of 5.60 atm and a volume of 12.0 liters?

a)

237 mL

b)

237 K

c)

237 L

d)

237 atm

52.

A 20.0 gram sample of hydrogen gas has a volume of 40.55 L and a tempeature of 67.00C. What is the pressure of the gas? (hint--don't forget to convert mass to moles!!)

a)

2.71 mm Hg

b)

2.71 atm

c)

6.88 mm Hg

d)

6.88 atm

53.
If the pressure exerted by a gas at 25 degrees C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?
a)
.002766 mole
b)
.0069 mol
c)
2.766 mol
d)
9.887 mol
54.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
55.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
56.

Which formula would you use to answer the following problem?

At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?

a)

PV=nRT

b)

P1V1/T1=P2V2/T2

c)

Not enough information is given.

57.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
58.
If the temperature of a gas increase, the pressure...
a)
Decreases
b)
Increases
c)
Does not change
59.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
60.

A gas at 928 kpa, 129 C occupies a volume of 569 L. Calculate the volume at 319 kpa and 32 C.

a)

1256 L

b)

418.18 L

c)

1100 L

d)

1400 L

61.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
62.
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
63.
What variable should be placed in the blank to complete the following expression of the ideal gas equation:  PV = nR___?  
a)
boiling point of the gas in Kelvins 
b)
temperature of the gas in Celsius
c)
temperature of the gas in Kelvins 
d)
density of the gas in g/cm3
64.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
65.

If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature, what is the new volume?

a)

23.2

b)

21.8

c)

0.0431

d)

0.0459

66.

A balloon is filled with 35.0 L of helium in the morning when the temperature is 20.0 degrees Celsius. By noon the temperature has risen an additional 25 degrees. What is the new volume of the balloon?

a)

38L

b)

79L

c)

44L

d)

36L

67.

6.0 L of gas in a piston at a pressure of 1.0 atm are compressed until the volume is 3.5 L. What is the new pressure inside the piston?

a)

1.7 atm

b)

0.6 atm

c)

21 atm

d)

1 atm

68.

A gas occupies 900.0 mL at 150 kPa. What is the new pressure when the gas is compressed to only 500.0 mL?

a)

270 kPa

b)

270 atm

c)

83 kPa

d)

83 atm

69.

If a gas is cooled from 323.0 K to 273.15 K and volume is kept constant, what final pressure would result if the original pressure was 750.0 mmHg?

a)

634 mmHg

b)

887 mmHg

c)

887 atm

d)

634 atm

70.

How many moles of helium are in a gas

sample that has a volume of .5 L at a

pressure of 3.00 atm and a temperature of

298 K?

a)

6.13 moles

b)

0.613 moles

c)

0.0613 moles

d)

61.3 moles

71.

How many moles of helium are contained in a 5.00L canister at 101kPa and 30.0oC?

a)

2.02 moles

b)

0.201 moles

c)

0.494 moles

d)

4.99 moles

72.

A water bottle at STP is cooled to -155°C. What is the new pressure?

a)

3.2 atm

b)

0.43 atm

c)

1.8 atm

d)

0.27 atm

73.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

74.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

75.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
76.
The temperature at which all molecular motion stops is
a)
-460 .C
b)
-273K
c)
0K
d)
0.C
77.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
78.
What pressure in kPa is equal to 2.65 atm?
a)
268 kPa
b)
0.0261 kPa
c)
39.0 kPa
d)
265 kPa
79.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
80.
What is the variable for this number 9.10 atm
a)
P
b)
T
c)
n
d)
V
81.
What is the variable for this number 122 K
a)
P
b)
T
c)
n
d)
V
82.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
83.

Which answer shows the correct Combined Gas Law

a)

P1V1T2=P2V2T1\frac{P_1V_1}{T_2}=\frac{P_2V_2}{T_1}

b)

P1V1T1=P2V2T2\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}

c)

P1V2T1=P2V1T2\frac{P_1V_2}{T_1}=\frac{P_2V_1}{T_2}

d)

P2V1T1=P1V2T2\frac{P_2V_1}{T_1}=\frac{P_1V_2}{T_2}

84.

A real gas differs from an ideal gas because the molecules of a real gas have

a)

A) Some volume and no attraction for each other

b)

B) Some volume and some attraction for each other

c)

C) No volume and no attraction for each other

d)

D) No volume and come attraction for each other

85.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
86.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

87.
Consider a sample of oxygen gas at 27° C with a volume of 9.55L at a pressure if 2.97 atm.  The pressure is changed to 8.25 atm and the gas is heated to 125° C.  What’s the new volume? 
a)
4.56 L
b)
4.6 L
c)
15.9 L
d)
16 L
88.

a)

this is a graph representing Boyle's law

b)

this is a graph representing Charles' law

c)

this is a graph representing Avogadro's law

d)

this is a graph representing ideal gas law

89.

a)

this is a graph representing Boyle's law

b)

this is a graph representing Charles' law

c)

this is a graph representing Avogadro's law

d)

this is a graph representing ideal gas law

90.

What is happening as you move from volume 1 to volume 2?

a)

The pressure is held constant

b)

There are the same number of molecules in a smaller container, so volume 2 will have a higher pressure because the molecules are hitting the sides more often.

c)

There are more molecules in volume 2, which would cause them to be hotter and move faster, therefore pressure is increased.

d)

Volume 1 would have a higher pressure.

91.

Which formula would you use to solve the following equation?

If I have 23 L of Ar at a pressure of 12 atm and a temperature of 200 K, and then I increase the pressure to 14 atm and the temperature to 300 K, what is my new volume?

a)

PV=nRT

b)

Not enough information is given.

c)

P1V1/T1 = P2V2/T2

92.

As pressure increases, volume decreases. Describe the relationship:

a)

Direct Relationship

b)

Inverse Relationship

c)

No Relationship

93.

As temperature increases, volume increases. Describe the relationship:

a)

Direct Relationship

b)

Inverse Relationship

c)

No Relationship

94.

As pressure increases, temperature increases. Describe the relationship:

a)

Direct Relationship

b)

Inverse Relationship

c)

No Relationship

95.
What is temperature?
a)
How much space an object takes up.
b)
A measure of how fast particles are moving.
c)
How much mass is in an object. 
96.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
97.
What about gasses can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
98.
If the atoms of an object are moving fast, the temperature would be...
a)
High
b)
Low
99.

Which equation would you use to solve the following problem:

"The volume of of 300 mL of gas at 1 atm is decreased to 100 mL. What is the new pressure?"

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1V1)/T1 = (P2V2)/T2

d)

None of the above

100.

Which equation would you use to solve the following problem:

"A gas occupies 2 L of space at 0 C. What will its volume be at 100 C?"

a)

P1V1 = P2V2

b)

V1/T1 = V2/T2

c)

(P1V1)/T1 = (P2V2)/T2

d)

None of the above

101.

Which equation do you use? "A 4L container at 298K contains 25 grams of carbon dioxide gas. What pressure is the container?"

a)

P1V1=P2V2

b)

P1 / T1=P2 / T2

c)

V1 / T1=V2 / T2

d)

PV=nRT

102.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know

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