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Gasses & Gas Laws

Total questions: 59

Worksheet time: 3hrs 20mins

Name
Class
Date
1.
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
2.
How are pressure and volume related?
a)
Directly
b)
Indirectly
c)
They aren't related
3.
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
4.
What law combines all 3 factors (pressure, temperature, and volume)
a)
Combined Gas Law
b)
Charle's Law
c)
Boyle's Law
d)
Avagadros Ideal Gas Law
5.

If a gas is measured to have a volume of 0.5atm at 273K, what would happen to the pressure if the temp increased to 300K?

a)

increase

b)

decrease

c)

remain the same

6.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
7.

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

8.

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

9.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
10.
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
11.

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.

12.
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
13.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
14.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
15.
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
16.
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
17.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
18.
As number of moles goes up, volume 
a)
goes down.
b)
goes up.
c)
stays the same
19.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
20.
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
21.
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 
22.

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

23.

How do you convert Celsius to Kelvin?

a)

Add 273

b)

Subtract 273

c)

They are the same thing

24.
If you increase the pressure of a constant volume of gas, what will happen to the temperature?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
25.

What is 50oC in Kelvin?

a)

223 K

b)

323 K

c)

100 K

d)

50 K

26.
What will happen to the volume of a gas under constant temperature if the pressure increases?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
27.
Which of the following has the greatest amount of movement at a given temperature?
a)
Gas
b)
Liquid
c)
Solid
d)
They all have the same movement
28.
Which of the following would increase the pressure on a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
29.
Which phase has the highest kinetic energy? 
a)
solid
b)
liquid 
c)
gas
d)
matter
30.

A balloon has 15.0 g of O2 at 27.0°C and 1.54 atm. What is the volume?

a)

.0675 L

b)

7.50 L

c)

15.0 L

d)

240 L

31.

A gas has a volume of 480 mL at 90.0 mmHg pressure. What pressure is needed to change the volume of the gas to 320 mL?

a)

60.0 mmHg

b)

80.0 mmHg

c)

100 mmHg

d)

135 mmHg

32.

If the pressure exerted by a gas at 25oC 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

33.

A sample of oxygen gas occupies a volume of 250 mL at 740 Torr pressure. What volume will it occupy at 800 Torr pressure?

a)

266 mL

b)

245 mL

c)

231 mL

d)

217 mL

34.

At 249 kPa sample of nitrogen is heated from 86oC to 107oC. What pressure will the sample have at the higher temperature?

a)

264 kPa

b)

266 kPa

c)

842 kPa

d)

824 kPa

35.
A sample of gas has a volume of 0.600 L at 30°C and a pressure of 0.8 atm. What is the number of moles in this sample?
a)
0.2 mol
b)
0.02 mol
c)
14.4 mol
d)
145.4 mol
36.

A 0.25 mol sample of neon gas at 18oC and 0.799 atm is heated to 49oC. The new gas pressure is 1.11 atm. What is the volume of the neon gas?

a)

30 L

b)

5.95 L

c)

7.47 L

d)

1.50 L

37.

What does R stand for in the ideal gas law?

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

38.

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

39.
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
40.
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
41.

What type of relationship to pressure and volume have?

a)

direct

b)

inverse

42.

What type of relationship to temperature and volume have?

a)

direct

b)

inverse

43.

What type of relationship to temperature and pressure have?

a)

direct

b)

inverse

44.

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10.0 L to 15.0 L. The final pressure is ___ atm.

a)

1.5 atm

b)

15 atm

c)

0.67 atm

d)

3.3 atm

e)

7.5 atm

45.

A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ___L at 423 K and 1.00 atm.

a)

0.709 L

b)

57.9 L

c)

41.1 L

d)

81.6 L

e)

1.41 L

46.

The density of N2O at 1.52 atm and 45.2ºC is ____ g/L.

a)

0.388 g/L

b)

2.58 g/L

c)

9.99 g/L

d)

1.76 g/L

e)

18.2 g/L

47.

The volume of a sample of gas (2.49 g) is 752 mL at 1.98 atm and 62ºC. What is the gas?

a)

NO2

b)

SO3

c)

SO2

d)

Ne

e)

NH3

48.

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide and 3.33 g of argon; all at 42ºC is ____ mmHg.

a)

116 mmHg

b)

395 mmHg

c)

134 mmHg

d)

263 mmHg

e)

0.347 mmHg

49.

Gases generally have

a)

low density

b)

high density

c)

closely packed particles

d)

no increase in volume when temperature is increased

e)

no decrease in volume when pressure is increased

50.

A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6°C. Determine the temperature at which the volume of the gas is 3.42 L.

a)

312K

b)

278K

c)

20.4K

d)

295K

e)

552K

51.

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

a)

H2

b)

He

c)

Ne

d)

O2

e)

All have the same volume.

52.
If container A is 10L and is under 5 atm of pressure and container B is 10L, but under 7 atm of pressure, what is true about the number of particles inside the containers?
a)
can not tell from the information
b)
they contain the same number of particles
c)
container A has less particles
d)
container B has less particles
53.
Consider the lab station with the syringe probe. When the volume of air decreased what happened to pressure?
a)
pressure increased due to increased kinetic energy of each gas particle
b)
pressure increased due to the smaller volume and more collisions with the sides of the syringe
c)
molecules collided less due to the pressure decreased due to smaller volume  of molecules
d)
pressure increased because molecules were moving faster due to the increase number of molecules
54.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

a)

0.13 atm

b)

0.27 atm

c)

0.63 atm

d)

0.90 atm

55.

The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127oC. What is the molar mass of this gas?

a)

(254/3) R

b)

188 R

c)

(800/3) R

d)

600 R

56.

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is

a)

28 mm Hg

b)

56 mm Hg

c)

133 mm Hg

d)

161 mm Hg

57.

At 25°C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate?

a)

O2 (molar mass 32 g/mol)

b)

He (molar mass 4.0 g/mol)

c)

CO2 (molar mass 44 g/mol)

d)

Cl2 (molar mass 71 g/mol)

58.

NH4NO3(s) → N2O(g) + 2 H2O(g)


A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol–1 K–1)

a)

3 atm

b)

1 atm

c)

0.5 atm

d)

0.1 atm

59.

A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0°C and 1.00 atmosphere. A possible formula for the hydrocarbon is

a)

CH2

b)

C2H4

c)

C3H6

d)

C4H8

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