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Gas Laws

Total questions: 76

Worksheet time: 2hrs 59mins

Name
Class
Date
1.
A gas that has a pressure of 2 atm and a volume of 10 L.  What would be the new volume if the pressure was changed to 1 atm?
a)
P1/T1 = P2/T2
b)
P1V1 = P2V2
c)
V1/n1 = V2/n2
d)
PV = nRT
2.
A sample of a gas has a volume of 852 mL at 298 K. What temperature is necessary for the gas to have a volume of 945 mL?
a)
Pt = P1 + P2 + P3 + ...
b)
P1V1 = P2V2
c)
V1/T1 = V2/T2
d)
P1V1/T1 = P2V2/T2
3.
If a nitrogen gas occupies a volume of 500 ml at a pressure of 0.971atm. What volume will the gas occupy at a pressure of 1.50 atm?  
a)
P1V1 = P2V2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/n1 = V2/n2
4.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
V1/n1 = V2/n2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/T1 = V2/T2
5.
A container is filled with H2, and H2O. What is the partial pressure of H2 when the pressure of water is 17 kPa. The total pressure of the gases is 750 kPa.
a)
P1V1 = P2V2
b)
Pt = P1 + P2 + P3 +...
c)
P1/T1 = P2/T2
d)
V1/n1 = V2/ n2
6.
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)
P1V1 = P2V2
b)
P1/T1 + P2/T2
c)
PV = nRT
d)
V1/T1 = V2/T2
7.
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
8.
A gas fills a balloon at a temperature of 27 oC and 1 atm of pressure. What will the pressure of the balloon be if the gas is heated to 127 oC?
a)
P1V1 = P2V2
b)
PV = nRT
c)
P1/T1 = P2/T2
d)
V1/T1 = V2/T2
9.
A 220.0 mL sample of helium gas is in a cylinder at 105 kPa and 275 K. The piston is pushed in until the sample has a new temperature of 310 K and new pressure of 150 kPa. What is the new volume of the gas? 
a)
P1V1/T1 = P2V2/T2
b)
PV = nRT
c)
P1V1 = P2V2
d)
Pt = P1 + P2 + P3 + ...
10.
A gas is at a pressure of 12 atm, a volume of 23 L, and a temperature of 200K. If the pressure is raised to 14 atm,  and the temperature is increased to 300K. What is the new volume of the gas?
a)
P1V1/T1 + P2V2/T2
b)
PV = nRT
c)
P1V1 = P2V2
d)
P1/T1 = P2/T2
11.
The gas in the container is at a pressure of 3.00 atm at 298 K.  What would be the pressure in the container at 325 K?
a)
P1/T1 = P2/T2
b)
P1V1 = P2V2
c)
V1/T1 = V2/T2
d)
PV = nRT
12.
A container has 0.504 moles of a gas at a volume of 2680 mL.  When the number of moles changes to 0.423 moles, what is the new volume?
a)
PV = nRT
b)
V1/n1 = V2/n2
c)
P1V1/T1 = P2V2/T2
d)
P1V1 = P2V2
13.
If the total pressure is 0.99 atm, and the partial pressure of carbon dioxide and hydrogen sulfide is 0.05 atm and 0.02 atm respectively.  What will be the partial pressure of the remaining air?
a)
P1V1 = P2V2
b)
Pt = P1 + P2 + P3 + ...
c)
PV = nRT
d)
P1/T1 = P2/T2
14.
A 1.25 L volume of gas contains 4.5 moles.  How many moles will be in 0.75 L?
a)
PV = nRT
b)
P1V1 = P2V2
c)
P1V1/T1 = P2V2/T2
d)
V1/n1 = V2/n2
15.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
16.
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
17.
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
18.
What is 0 Kelvin known as
a)
No such thing
b)
Very cold
c)
Freezing point of Water
d)
Absolute Zero
19.
If the temperature of a gas increase, the pressure...
a)
Decreases
b)
Increases
c)
Does not change
20.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
21.
In the ideal gas law, what does the variable n represent? 
a)
gas constant 
b)
moles 
c)
Temperature 
d)
Volume 
22.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
23.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
24.
Which of the following is NOT a value for standard pressure?
a)
101.3 kPa
b)
760 mm Hg
c)
1 atm
d)
1 torr
25.
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
a)
204 K
b)
200 K
c)
2046 K
d)
2000 K
26.
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
27.
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
28.
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
29.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
30.
If the temperature of a gas increase, the pressure...
a)
Decreases
b)
Increases
c)
Does not change
31.
Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 
a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
32.

What describes the motion of a Gas Molecule?

a)

Molecules are far apart

b)

Move in constant, random motion

c)

It will travel in a straight path

d)

All of the above

33.

If pressure goes down in a container, what happens to volume when the temperature is held constant.

a)

Increase

b)

Decrease

34.

If temperature goes down in a container, what happens to volume when the pressure is held constant.

a)

Increase

b)

Decrease

35.

If you add gas particles to the container, what happens to the volume when the pressure and temperature is held constant.

a)

Increase

b)

Decrease

36.

How would you convert 34oC to Kelvin?

a)

K = oC + 273

b)

oC = K + 273

c)

K = oC - 273

d)

oC = K + 273

37.

What formula would you use to solve the following: A 0.562 L container of Helium has a pressure of 9.5 atm. What volume would be necessary to decrease the pressure to 2.4 atm?

a)
b)
c)
d)
38.

What formula would you use to solve the following: A sample of nitrogen gas was collected over water at a temperature of 23.0°C. What is the partial pressure of nitrogen if the atmospheric pressure (total) was 785 mmHg and the vapor pressure of water was 21.1 mmHg?

a)
b)
c)
d)
39.

What formula would you use to solve the following: A container of carbon monoxide gas is at a temperature of 65.0 °C and occupies a volume of 6.5L. At what temperature would it occupy a volume of 10.2L?

a)
b)
c)
d)
40.

What formula would you use to solve the following problem: A gas at 880mmHg and 298K occupies a container with an initial volume of 1.00 L. The pressure increases to 1980mmHg as the temperature rises to 398K. What will be the new volume?

a)
b)
c)
d)
41.

What formula would you use to solve the following: At high altitudes, pilots have to supplement their supply of oxygen. In this mixture, there are oxygen and nitrogen gases. If nitrogen’s partial pressure is 250mmHg, calculate the partial pressure of oxygen if the total pressure is 710mmHg.

a)
b)
c)
d)
42.

What formula would you use to solve the following: 6.25L of nitrogen gas is known to contain 5.21 moles. If the amount of nitrogen is increased to 12.64 moles, what new volume will result (at unchanged temperature and pressure)?

a)
b)
c)
d)
43.

What formula would you use to solve the following problem: A container has an initial volume of 4.5 L, a pressure of 450 kPa and is at a temperature of 15oC. If the container is expanded to 6.5 L while the pressure is decreased to 125 kPa, find the resulting temperature.

a)
b)
c)
d)
44.

What formula would you use to solve the following question: How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of

12.4 atm and a temperature of 850 C?

2H2(g) + O2(g) --> 2H2O(l)

a)
b)

STOICH and PV = nRT

c)
d)
45.

What formula would you use to solve the following: If a cylinder has a volume of 5.4 x 106 L of air at a pressure of 140 kPa and it is determined that there are 3.0 x 105 moles of CO2 present, calculate the temperature inside the cylinder.

a)
b)
c)
d)
46.

What formula would you use to solve the following problem: 76 L of compressed oxygen is at a temperature of 330 K. If there are 7.3 moles of oxygen in the container, calculate the pressure (in atm) inside the container.

a)
b)
c)
d)
47.

Which of the following is NOT a unit of Pressure?

a)

mmHg

b)

atm

c)

kelvin

d)

psi

48.

Which Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagodro's Law

d)

Combined Gas Las

49.

What Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagadro's Law

d)

Combined Gas Law

50.

In the Question: A cylinder has a volume of 5.4 L of air at a pressure of 140 atm. If the volume is increased to 12.4L, what would the new pressure be? Which answer choice has the data correctly labeled?

a)

P1=5.4L, V1=140atm; P2= 12.4L, V2= ?

b)

P1=140atm, V1=5.4L ; P2= ?, V2=12.4L

c)

T1=140atm, V1=5.4L ; T2= ?, V2=12.4L

d)

There was no important data to label

51.

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

52.

What will happen to the volume of a gas under constant pressure if the temperature increases?

a)

Decrease

b)

Explosion!

c)

Increase

d)

Nothing

53.

What does the kinetic theory states?

a)

At the same temperature the object that has the most mass heats quicker.

b)

Particles won't move if you don't apply energy to it.

c)

Particles only move in liquids and gases.

d)

Particles are always in motion.

54.

A sample of oxygen gas in a closed system has a volume of 200 L at 600 K. If the pressure is held constant and the temperature is lowered to 300 K, what will be the new volume of the gas?

a)

100 L.

b)

200 L.

c)

300 L.

d)

400 L.

55.

A 2.0 liter container of nitrogen had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm?

a)

5 L

b)

6.4 L

c)

6.9 L

d)

7.2 L

56.

A sample of carbon dioxide occupies a volume of 3.50 liters at 1.25 atm of pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters?

a)

2.19 atm

b)

2.22 atm

c)

5.67 atm

d)

6.54 atm

57.

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

a)

21.8 L

b)

23.2 mm Hg

c)

23.2 L

d)

21.8 ∘C

58.

A 40.0 L tank of ammonia has a pressure of 12.7 kPa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kPa while its temperature remains constant.

a)

60.5 L

b)

60.5 kPa

c)

26.5 L

d)

2.67 L

59.
Which gas law allows us to look at how three different properties of a gas change simultaneously?
a)
Combined Gas Law
b)
Charles's Law
c)
Ideal Gas Law
d)
Boyle's Law
60.
Which gas law allows us to solve for one unknown property of a gas, without changing any properties of the gas?
a)
Avogadro's Law
b)
Charles's Law
c)
Ideal Gas Law
d)
Combined Gas Law
61.

Two flasks containing different gases but are both at the same temperature and the same pressure. One flask contains 10.0 g of Ne and the other flask contains 8.0 g of He. Which of the following statements are correct?

a)

Both flasks contain the same number of atoms

b)

The volume of the flasks must be the same

c)

The flask containing helium has a higher volume than the flask that contains neon

d)

The kinetic energy for He is higher than kinetic energy of Ne.

62.

Which of the following equations is Boyle’s Law?

a)

P1V1= P2V2P_1V_1=\ P_2V_2

b)

P1T1=P2T2\frac{P_1}{T_1}=\frac{P_2}{T_2}

c)

V1n1=V2n2\frac{V_1}{n_1}=\frac{V_2}{n_2}

d)

V1T1=V2T2\frac{V_1}{T_1}=\frac{V_2}{T_2}

63.

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)

2.3 atm

c)

1.6 atm

d)

3.4 atm

64.
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
65.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
rubber in the tires reacts with oxygen in the atmosphere
c)
air molecules speed up and collide with the tire walls more often
d)
air molecules diffuse rapidly through the walls of the tire.
66.

Lord Kelvin derived the temperature at which (theoretically) all kinetic energy is removed and molecules stop moving. What temperature, in Celsius, is absolute zero?

a)

O°C

b)

-273°C

c)

273°C

d)

0K

67.

Lord Kelvin derived the temperature at which (theoretically) all kinetic energy is removed and molecules stop moving. What temperature, in Celsius, is absolute zero?

a)

O°C

b)

-273°C

c)

273°C

d)

0K

68.

Which of the following does not describe molecules in the Kinetic Molecular Theory?

a)

Molecules are in constant, random motion.

b)

There are no interactions between molecules.

c)

More heat means more kinetic energy.

d)

Collisions between molecules are elastic and lose no energy.

e)

Molecules take a definite shape and have no volume.

69.

The volume of a gas at 99.0 kPa is 300. mL. If the pressure is increased to 188 kPa, what will be the new volume?

a)

158 mL

b)

570 mL

c)

273 mL

d)

-132 mL

70.

A gas at 89°C occupies a volume of 0.67 L. At what Celsius temperature will the volume increase to 1.12 L?

a)

330°C

b)

603°C

c)

148°C

d)

273°C

71.

The pressure in an automobile tire is 1.88 atm at 25°C. What will be the pressure if the temperature increases to 37°C?

a)

1.96 atm

b)

2.78 atm

c)

273 atm

d)

1.22 atm

72.

A sample of air in a syringe exerts a pressure of 1.02 atm at 22°C. The syringe is placed in a boiling-water bath at 100°C. The pressure is increased to 1.23 atm by pushing the plunger in, which reduces the volume to 0.224 mL. What was the initial volume?

a)

0.214 mL

b)

1.23 mL

c)

2.11 mL

d)

2.73 mL

73.

The pressure of a sample of helium in a 1.00-L container is 0.988 atm. What is the new pressure if the sample is placed in a 2.00-L container?

a)

0.494 atm

b)

2.02 atm

c)

1.98 atm

d)

2.73 atm

74.

The Celsius temperature of a 3.00-L sample of gas is lowered from 80°C to 30°C. What will be the resulting volume of this gas?

a)

2.58 L

b)

1.13 L

c)

16.7 L

d)

273 L

75.

Helium gas in a 2.00-L cylinder is under 1.12 atm pressure. At 36.5°C, that same gas sample has a pressure of 2.56 atm. What was the initial temperature in degrees Celsius of the gas in the cylinder?

a)

-138°C

b)

15.9°C

c)

-14.8°C

d)

273°C

76.

A balloon contains 146.0 mL of gas confined at a pressure of 1.30 atm and a temperature of 5.0°C. If the pressure doubles and the temperature decreases to 2.0°C, what will be the volume of gas in the balloon?

a)

72 mL

b)

273 mL

c)

175 mL

d)

321 mL

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