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Gas Law Review

Total questions: 102

Worksheet time: 9hrs 30mins

Name
Class
Date
1.
Gas laws involve what three variables?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
2.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
3.
What will happen to the volume of a gas if the pressure increases, with constant temperature ?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
4.
If you increase the pressure, what will happen to the temperature, if volume is constant?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
5.
According to the Combined Gas Law, pressure and volume are inversely related which means that
a)
When pressure increases, volume increases
b)
When pressure decreases, volume decreases
c)
When pressure increases, volume decreases
d)
When pressure doubles, volume triples
6.
According to the Combined Gas Law, volume and temperature are directly related. This means that
a)
When volume increases, temperature increases
b)
When volume increases, temperature decreases
c)
When volume double, pressure triples
d)
When volume doubles, volume is reduced by 1/2
7.
If 6L of gas at 293K is compressed to 4L, what is the new temperature? 
a)
195K
b)
439.5K
c)
0.082K
d)
12.2K
8.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
9.
4L of a gas is contained at 300 kPa and 200K. What will its volume be in L at 140 kPa and 100K?
a)
4.3L
b)
4.8L
c)
6.2L
d)
8.5L
10.
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)
1255 L
d)
1400 L
11.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
12.
Using Combined Gas Law, if the pressure of a gas starts out at 200kPa and increases to 600kPa, what would the initial temperature be if it ended up at 300K?
a)
50K
b)
200K
c)
400K
d)
100K
13.
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
14.
The temperature at which all molecular motion stops is
a)
-460 .C
b)
-273K
c)
0K
d)
0.C
15.
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.
16.
The random molecular motion of a substance is greatest when the substance is
a)
condensed
b)
frozen
c)
gas
d)
a liquid
17.
The kinetic theory of matter states that all of the particles that make up matter are constantly
a)
growing
b)
shrinking
c)
crying
d)
moving
18.
At higher temperatures...
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
19.
If you place a balloon in a freezer what happens to the size of the balloon?
a)
Doubles
b)
increases
c)
decreases
d)
stays still
20.

Which is NOT a unit of Pressure

a)

atm

b)

mmHg

c)

Liters

d)

kPa

21.

The following graph illustrates what kind of RELATIONSHIP between pressure and temperature?

a)

Direct

b)

Inverse

c)

Indirect

d)

Negative Slope

22.

The following graph illustrates what kind of Relationship between Pressure and Volume?

a)

Direct

b)

Positive Slope

c)

Indirect

d)

As pressure increases, volume increases

23.

A sample of oxygen under 2.5 atm pressure occupies 1.5 Liters. What volume will it occupy at 7 atm? (2 decimal places)

(a)  

24.

A gas has a pressure of 500 mmHg at 200 K. What is the temperature at 750 mmHg?

(a)  

25.

What change in volume results if 65 mL of gas is cooled from 353 K to 323 K? (2 decimal places)

(a)  

26.

Convert 30 degree Celsius to Kelvin

a)

303 K

b)

-243 K

c)

8190 K

d)

9.1 K

27.

On a cold day near the ocean, it was found that 8g of an unknown gas occupies a volume that is little less than 6L. based on this information, which if the most likely identity of the unknown gas?

a)

CO2

b)

Ne

c)

O2

d)

CH4

28.

Which of the following gases is expected to behave most ideally at a given temperature and pressure?

a)

H2O

b)

NH3

c)

Xe

d)

He

29.

An experiment is performed to measure the pressure of chlorine gas with in a 2.00L container at 273K. The student calculates the pressure using the ideal gas law to be 67.2atm. They calculated the pressure again using the van der Waals equation for real gases to be 22.5atm. What is the major factor that accounts for the difference between these two values?

a)

Chlorine is a halogen

b)

Diatomic nature of chlorine

c)

Volume of the chlorine particles

d)

Forces of attraction between chlorine molecules

30.

A sample of gas is heated from 35oC to 70oC. Which statement correctly describes what happens to the volume?

a)

The volume increases by a factor of less than 2

b)

The volume increases by a factor of 2

c)

The volume decreases by a factor of less than 2

d)

The volume decreases by a factor of 2

31.

What is the total pressure produced in this explosion?

a)

25.0atm

b)

52.0atm

c)

179atm

d)

435atm

32.

In a second experiment, the total pressure is observed to be 58atm. What is the partial pressure of the water vapor produced?

a)

10atm

b)

20atm

c)

30atm

d)

40atm

33.

Two gases are removed from their original containers and placed into a third container, where they react with each other. All three containers have identical volumes, and all gases are at the same temperature. Which container has the lowest pressure?

a)

Container A before the reaction

b)

Container B before the reaction

c)

Container C after the reaction

d)

they all have the same pressure

34.

Which of the following is a reasonable estimate for the volume of a balloon that has been filled with 300g of oxygen gas at STP?

a)

1 L

b)

10 L

c)

50 L

d)

200 L

35.

CH4 --- N2 --- CO --- SO2 --- From the gases listed, 1.00 mol of each of two different gases are placed simultaneously into a container with a small pinhole. Which combination of gases would result in the greatest difference rate of effusion and why?

a)

SO2 and CH4 because their molar masses are the largest and smallest, respectively

b)

CO and SO2 because sulfur's 3p electrons are further from the nucleus than the 2p electrons in carbon.

c)

N2 and CO because they both have pi bonding which results in a shorter bond length between the atoms of each molecule.

d)

CO and SO2 because the linear shape of CO allows it to pass through the pinhole easily while the bent shape of SO2 prohibits it from effusing.

36.

Two identical railroad tank cars are evacuated and each is then filled with 1.2x103 moles of a gas at 27oC. Tank car #1 is filled with sulfur dioxide, which Tank car #2 is filled with carbon monoxide. Initially the pressures in the tanks are equal. During a train derailment, identical pin-sized holes are made in each tank car; the decrease in pressure of each tank car is monitored. One of the tank cars has a much more rapid decrease in pressure than the other. Which statement best explains this?

a)

The pressure in Tank car #1 decreases more rapidly because the heavier molecules of SO2 have a greater velocity than that of CO molecules.

b)

The pressure in Tank car #1 decreases more rapidly because there are more molecules of SO2 than molecules of CO.

c)

The pressure in Tank car #2 decreases more rapidly because CO molecules are lighter and have a higher velocity than SO2 molecules

d)

The pressure in Tank car #2 decreases more rapidly because there are more molecules of CO than molecules of SO2

37.

According to the Kinetic Molecular Theory a liquid's (SELECT ALL THAT APPLY)

a)

particles are held close together by intermolecular forces

b)

particles are in constant motion

c)

particles are vibrating in place and closely packed

d)

particles are not moving

38.

The properties of liquids include (SELECT ALL THAT APPLY)

a)

definite volume

b)

take the shape of the container

c)

can flow

d)

are relatively incompressible

e)

can diffuse and have surfacre tension

39.

Which of the following is an assumption of the kinetic-molecular theory of gases?

a)

Collisions between gas particles are inelastic.

b)

Gases consist of closely spaced particles.

c)

Gas particles move around in an orderly manner.

d)

The temperature of a gas depends on the average kinetic energy of the gas particles.

40.

Which of the following is the equation needed to calculate the kinetic energy, KE, of a moving particle?

a)

KE = 1/2 mv2

b)

KE = 2mv

c)

KE = mv

d)

KE = 1/2 m2v

41.

If a gas has the same temperature throughout, which gas molecule has the highest average velocity?

a)

O2

b)

H2O

c)

H2

d)

Xe

42.

Which condition is necessary for most gases to behave nearly ideally?

a)

high pressure

b)

high temperature

c)

low compressibility

d)

low expansion

43.

Which of the following is not a physical property of gases?

a)

absence of definite volume

b)

large density

c)

high compressibility

d)

fluidity

44.

Which states of matter are fluid?

a)

gases and liquids

b)

liquids and solids

c)

gases only

d)

liquids only

45.

Which gas deviates the most from ideal behavior?

a)

CH4

b)

H2O

c)

Cl2

d)

He

46.

The pressure exerted by a gas does not depend on

a)

temperature.

b)

volume.

c)

number of moles present.

d)

the identity of the gas.

47.

The energy of motion is known as ___.

a)

potential energy

b)

kinetic energy

c)

mechanical energy

48.

The pressure of each flask is given in atmospheres (atm). Flask 1 has the lowest pressure, and Flask 4 has the highest. Knowing what causes gas pressure, which of the following statements is true?

a)

Flask 1 contain the most molecules

b)

Flask 2 contain the most molecules

c)

Flask 3 contain the most molecules

d)

Flask 4 contain the most molecules

49.

Which of the following statements is true?

a)

Gases do not move in straight line

b)

Gas particles are spaced so far apart that most of the volume of gas is empty space

c)

Gas particles are not in constant motion

d)

Gas particles attract each other

50.
Of these three states of matter, which one has the most kinetic energy? 
a)
Solid 
b)
Liquid 
c)
Gas
51.

Adding heat to a solid makes the particles move...

a)

Particles in a solid are not moving

b)

Slower

c)

At the same rate as before the heat was applied

d)

Faster

52.

The particles in a gas are ______ away from each other than the particles in a solid

a)

farther

b)

closer

c)

the same distance

53.

Which among the following is NOT true regarding the Kinetic Molecular Theory of gases?

a)

Gases particles move in straight lines.

b)

Gas particles are closely packed and their motion is orderly.

c)

Gas particles are in constant motion.

d)

Gas particles do not attract or repel each other.

54.
At what temperature do nitrogen molecules move fastest?
a)
350 K
b)
300 K
c)
250 K
d)
200 K
55.

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.

56.
The movement of gas molecules is greatly affected by _________.
a)
the shape of the container
b)
size of the container
c)
temperature of the container
57.

the forces that hold atoms together within a molecule.

a)

Velcro

b)

Intermolecular forces

c)

Intramolecular forces

d)

Polarity

58.

It is a type of chemical bond that generates two oppositely charged ions.

a)

Ionic bond

b)

Covalent Bond

c)

Dipole

d)

Ion-dipole

59.

These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.

a)

Dipole-dipole interaction

b)

Hydrogen bonding

c)

London Dispersion Forces

d)

ion-dipole interaction

60.

These are the weakest of the intermolecular forces and exist between all types of molecules, whether ionic or covalent—polar or nonpolar.

a)

Dipole-Dipole interaction

b)

London Dispersion

c)

Hydrogen Bonding

d)

Ion - dipole interaction

61.

The temperature of a substance is a measure of the average kinetic energy of the particles.

a)

True

b)

False

62.

Diffusion is the movement of particles from a high concentration to a low concentration.

a)

True

b)

False

63.

Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmospheres?

a)

0.217 atm

b)

0.466 atm

c)

0.613 atm

d)

1.63 atm

64.

"The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gases" is a statement of __________________ Law.

a)

Graham's

b)

Boyle's

c)

Avogadro's

d)

Dalton's

65.

Which of the lines on the figure is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant?

a)

a

b)

b

c)

c

d)

d

e)

e

66.

Which of the lines on the figure is the best representation of the relationship between the volume of a gas and its absolute temperature, other factors remaining constant?

a)

a

b)

b

c)

c

d)

d

e)

e

67.

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

a)

a

b)

b

c)

c

d)

d

e)

e

68.
Gases are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
69.
Liquids are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
70.
Solids are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
71.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
72.
In which state does matter completely fill its closed container?
a)
Gas
b)
Liquid
c)
Solid
d)
Ice
73.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
74.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
75.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
76.
How many moles are in 19.82 g Mg? 
a)
1.226mol Mg
b)
481.7mol Mg
c)
1.000mol Mg
d)
 0.82 mol Mg
77.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
78.
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
79.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

80.

1Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

81.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
82.
What is the mole ratio in the following reaction:
2CO  +  O2  → 2CO2
a)
2:1:2
b)
1:1:1
c)
1:2:1
d)
Have no clue what a mole ratios is!!
83.
1 mole of any gas at STP has a volume of ______________________. 
a)
22.4 liters
b)
44.2 liters
c)
6.02 x 1023 liters
d)
2.4 liters
84.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron (Fe) can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
85.

How many liters of N2, at STP, will react with 53.0 g H2 to form ammonia?


N2 + 3H2 --> 2NH3

a)

396 L

b)

17.6 L

c)

196 L

d)

588 L

86.

How many liters of SO2 will be produced from 55.0 L of O2 at STP?


2H2S + 3O2 --> 2SO2 + 2H2O

a)

55.0 Liters

b)

36.7 Liters

c)

18398 Liters

d)

2.45 Liters

87.

A sample of 3.0 grams of an ideal gas at 127°C and 1.0 atm has a volume of 1.5 L. What is the molar mass of this gas

a)

7.3 g/mol

b)

0.015 g/mol

c)

0.00092 g/mol

d)

66 g/mol

88.

If 0.20 mol of sulfur dioxide gas combines with 0.10 mol of oxygen gas to produce sulfur trioxide gas, what will the overall pressure in the flask be if the temperature is 25°C and the total volume is 4.0 L?

a)

0.61 atm

b)

1.2 atm

c)

0.051 atm

d)

0.10 atm

89.

At approximately what temperature will 40. g of argon gas at 2.0 atm occupy a volume of 22.4 L?

a)

1200 K

b)

1100 K

c)

550 K

d)

280 K

90.

A 1.00 L sample of a gas has a mass of 1.25 g at STP. What is the mass of 1.00 mol of this gas?

a)

0.855 g

b)

22.4 g

c)

1.25 g

d)

28.0 g

91.

A gas sample with a mass of 12.8 g exerts a pressure of 1.2 atm at 15°C and a volume of 3.94 L. What is the molar mass of the gas?

a)

19 g/mol

b)

32 g/mol

c)

64 g/mol

d)

128 g/mol

92.

A butane-fueled (combustion of C4H10) torch has a mass of 876.2 g. After burning for some time, the torch has a mass of 859.3 g. What volume of CO2 , at STP, was formed while the torch burned?

a)

1.63 L CO2

b)

9.93 L CO2

c)

9.93 L O2

d)

26.0 L CO2

93.

Aqueous sodium chloride, liquid water, gaseous carbon dioxide, and gaseous ammonia can be combined to form solid sodium bicarbonate and aqueous ammonium chloride. What volume of carbon dioxide compressed in a tank at 5.50 atm and a temperature of 42°C, will be needed to produce 100.0 kg of sodium bicarbonate?

a)

5.60 L CO2

b)

5.60 x 103 L CO2

c)

0.746 L CO2

d)

7.46 x 102 L CO2

94.

Hydrogen and oxygen react under a specific set of conditions to produce water according to the follwoing: 2H2(g) + O2(g) --> 2H2O(g). How many moles of hydrogen would be required to produce 5.0 mol of water?

a)

5.0 mol H2

b)

4.0 mol H2

c)

7.0 mol H

d)

5.0 mol of H

95.

If 4.50 mol of ethane, C2H6, undergo combustion according to the unbalanced equation C2H6 + O2 --> CO2 + H2O, how many moles of oxygen are required?

a)

16.8 mol O2

b)

15.8 mol O2

c)

16.0 mol O2

d)

15.9 mol O2

96.

Convert the following in a pressure reading expressed in torr: 1.25 atm

a)

1.25 torr

b)

608 torr

c)

126.65625 torr

d)

905 torr

97.

Convert the following into the unit specified: 125 mm Hg into atm.

a)

95000 atm

b)

0.165 atm

c)

6.08 atm

d)

950 atm

98.

Convert the following into the unit specified: 3.20 atm into Pa

a)

3.24 x 104 Pa

b)

3.2424 Pa

c)

3,242.4 Pa

d)

3.24 x 105 Pa

99.

Convert the following into the unit specified: 5.38 kPa into torr

a)

4088.8 torr

b)

141.26 torr

c)

40.4 torr

d)

131.03 torr

100.

A sample of gas at 47 degrees C and 1.03 atm occupies a volume of 2.20 L. What volume would this gas occupy at 107 degrees C and 0.789 atm?

a)

3.41 L

b)

5.01 L

c)

17.8 L

d)

0.09 L

101.

The pressure exerted on a 240. mL sample of hydrogen gas at consatnt temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?

a)

142 L

b)

142 mL

c)

0.1419 L

d)

141.878453 mL

102.

At standard temperature, a gas has a volume of 275 mL. The temperature is then increased to 130 degrees C, and the pressure is held constant. What is the new volume?

a)

305 mL

b)

186 mL

c)

406 mL

d)

400 mL

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