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Gas Laws Review

Total questions: 39

Worksheet time: 53mins

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 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
6.
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
7.
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
8.
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 + ...
9.
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
10.
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
11.
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
12.
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
13.

How would you convert 34oC to Kelvin?

a)

K = oC + 273

b)

oC = K + 273

c)

K = oC - 273

d)

oC = K + 273

14.

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)
15.

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)
16.

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)
17.

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)
18.

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)
19.

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)
20.

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)
21.

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)
22.

Which of the following is NOT a unit of Pressure?

a)

mmHg

b)

atm

c)

kelvin

d)

psi

23.

Which Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagodro's Law

d)

Combined Gas Las

24.

What Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagadro's Law

d)

Combined Gas Law

25.

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

26.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
27.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
28.
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
29.
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
30.
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
31.
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
32.

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

33.

Avogadro's Law explains the relationship between

a)

Pressure and Volume

b)

Pressure and Temperature

c)

Volume and Temperature

d)

Volume and Moles

34.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
35.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
36.
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 
37.
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
38.
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
39.
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 + ...

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