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Worksheets

END OF MODULE 12 REVIEW

Total questions: 119

Worksheet time: 3hrs 33mins

Name
Class
Date
1.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
2.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
3.

For the problem below, what is the value for the final pressure?

A gas with a volume of 4.0 L at 90.0 kPa expands until the pressure drops to 20.0 kPa. What is its new volume if the temperature doesn’t change?

a)

14.0 L

b)

20.0 L

c)

90.0 L

d)

18.0 L

4.

Suppose a balloon (volume 250.0 L) is inflated on a jet airplane at an altitude of 45,000 feet. The cabin of the airplane is pressurized to 0.75 atm. When the person with the balloon exits the air craft what will likely happen to the volume of the balloon? (Assume temp is same in and out of the plane).

a)

Stay the same since temp stays constant

b)

Enlarge

c)

Get smaller

d)

Unable to be predicted, too many variables.

5.
The pressure on a sample of gas is increased from 1.0 atm to 3.0 atm. If the new volume is 0.52 L, find the original volume.
a)

1.25 L

b)

1.56 L

c)

0.173 L

d)

None of these is very close.

6.

If a gas occupies a volume of 7.0 L at 273 K, what will be its volume at 473 K, assuming constant pressure?

a)

4.8 L

b)

6.4 L

c)

8.0 L

d)

12.1 L

7.

If the volume of a gas is 4.0 L at 400 K, what will be its volume at 600 K, assuming constant pressure?

a)

2.0 L

b)

4.0 L

c)

6.0 L

d)

8.0 L

8.

A balloon has a volume of 500 mL at a temperature of 300 K. If the temperature decreases to 150 K, what will be the new volume, assuming constant pressure?

a)

250 mL

b)

333 mL

c)

501 mL

d)

750 mL

9.
A gas has a volume of 2.5 L at 10°C. If the temperature is increased to 100°C, what will be its new volume, assuming constant pressure?
a)

1.25 L

b)

3.3L

c)

5.0 L

d)

2.5 L

10.

If a gas occupies a volume of 8.0 L at 300 K, what will be its volume at 400 K, assuming constant pressure?

a)

4.3 L

b)

10.7 L

c)

12.6 L

d)

16.0 L

11.

A gas is initially at a volume of 3.0 L at 25°C. If the volume is reduced to 2.3 L, what will be the new temperature of the gas, assuming constant pressure?

a)

-16.7°C

b)

-25.8°C

c)

-44.5°C

d)

-75°C

12.
A balloon has a volume of 500 mL at a temperature of 300 K. If the temperature decreases to 200 K, what will be the new volume, assuming constant pressure?
a)

250.6 mL

b)

333.3 mL

c)

524.5 mL

d)

750 mL

13.

Under what conditions is a real gals like and ideal gas?

a)

High temperature, high pressure

b)

Low temperature, high pressure

c)

High temperature, low pressure

d)

Low temperature, high pressure

14.

If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)

1.29 L

b)

12.36 L

c)

1.29 atm

d)

12.36 atm

15.

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)

1.8 atm

b)

2.27 atm

c)

1.8 L

d)

3.27 atm

16.
Gas laws involve what three variables?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
17.

What happens to pressure when temperature decreases

a)

increase in pressure

b)

decrease in pressure

c)

no change

18.

what relationship does this graph show?

a)

temperature and pressure- direct

b)

temperature and pressure- inverse

c)

pressure and volume- direct

d)

pressure and volume- inverse

19.
a)
This is an example of Charles's law
b)
This is an example of Boyle's law
20.
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
21.

Which rigid cylinder contains the same number of gas molecules as a 2.0 Liter rigid cylinder containing hydrogen gas?

a)

1.0 L of Oxygen gas

b)

2.0 L of methane gas

c)

1.5 L of ammonia gas

d)

4.0 L of Helium gas

22.
Review: Convert 48 g of fluorine gas to mol.
a)
19 mol
b)
22.4 mol
c)
0.776 mol
d)

1.26 mol

23.
Review: Convert 5.24 mol of hydrogen gas to liters. 
a)
0.00852 L
b)
117 L
c)
22.4 L
d)
2.00 L
24.

Review: Convert 35.0 L of oxygen gas to grams.

a)
25.0 g
b)
50.0 g
c)
0.020 g
d)
16.0 g
25.
If 1.00 mol of He occupies 22.4 L at STP, what volume will 1.00 g of He occupy under same condition?
a)
22.4 L
b)
5.60 L
c)
10.2 L
d)
8.16 L
26.
If 3.25 mol of Ar occupies 100. L at a particular temp and pressure, what volume does 14.15 mol of Ar occupy under same condition?
a)
435 L
b)
225 L
c)
100 L
d)
522 L
27.

Review: Convert 30 g of NO2 gas to mol.

a)

1.9 mol

b)

2.4 mol

c)

0.76 mol

d)

0.65 mol

28.

Review: Convert 5.24 mol of hydrogen gas to liters at STP.

a)
0.00852 L
b)
117 L
c)
22.4 L
d)
2.00 L
29.
If 1.00 mol of He occupies 22.4 L at STP, what volume will 1.00 g of He occupy under same condition?
a)
22.4 L
b)
5.60 L
c)
10.2 L
d)
8.16 L
30.

If you have 100 L of Argon at a particular temp and pressure, how many atoms of argon are there?

a)

2.78×10142.78\times10^{14} atoms

b)

4.8×10234.8\times10^{23} atoms

c)

2.69×10242.69\times10^{24} atoms

d)

266 atoms

31.

If 1.25 mol of N2 occupies 27.0 L at a particular temp and pressure, what volume does 0.89 mol of N2 occupy under the same conditions?

a)

20.0 L

b)

22.5 L

c)

10.0 L

d)

52.2 L

32.
Molar volume of any gas at STP
a)
22.4 L
b)
2.24 L
c)
6.02 x 1023 L
d)
224 L
33.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
34.

Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa.  (Use R = 8.314)

a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
35.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
36.
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
37.

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? (Use R = 0.0821)

a)
.002766 mole
b)
.0069 mol
c)
2.766 mol
d)
9.887 mol
38.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
39.

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm. (Use R = 0.0821)

a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
40.

Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. (Use R = 0.0821)

a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
41.

A hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory is known as

a)

real gas

b)

ideal gas

c)

imaginary gas

d)

perfect gas

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.

Under which conditions of temperature and pressure does carbon dioxide behave most like an ideal gas?

a)

A) Low temperature and low pressure

b)

B) Low temperature and high pressure

c)

C) High temperature and low pressure

d)

D) High temperature and high pressure

46.

Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas?

a)

A) 100K and 0.25 atm

b)

B) 100K and 25 atm

c)

C) 400K and 0.25 atm

d)

D) 400K and 25 atm

47.

One reason that a real gas deviates from an ideal gas is that the molecules of a real gas have

a)

A) a straight-line motion

b)

B) no net loss of energy on collision

c)

C) a negligible volume

d)

D) forces of attraction for each other

48.

A real gas behaves least like an ideal gas under the conditions of

a)

A) low temperature and low pressure

b)

B) low temperature and high pressure

c)

C) high temperature and low pressure

d)

D) high temperature and high pressure

49.

A sample of chlorine gas is at 300K and 1.00 atmosphere. At which temperature and pressure would the sample behave more like an ideal gas?

a)

A) 0 K and 1.0 atm

b)

B) 150 K and 0.50 atm

c)

C) 273 K and 1.00 atm

d)

D) 600 K and 0.50 atm

50.

What is the molar mass of B2(CO3)3?

a)

81.632 g/mol

b)

94.842 g/mol

c)

38.822 g/mol

d)

201.648 g/mol

51.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
52.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
53.
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
54.
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
55.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
56.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
57.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
58.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
59.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
60.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
61.
What is the percent yield of the following reaction if 145g of P2O5 reacts with 40 grams of water, but you only collected 112 grams of phosphoric acid? 3 H2O + P2O5 -> 2H3PO4
a)
80%
b)
85%
c)
77%
d)
58%
62.
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
63.
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
64.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
65.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
66.

Silicon dioxide, also known as silica, is an oxide of silicon with the chemical formula SiO2. Silica is one of the most complex and most abundant families of materials, existing as a compound of several minerals and as synthetic product. What is the formula mass of the covalent compound silicon dioxide (SiO2)?

a)

7193.6 amu

b)

30.0 amu

c)

44.1 amu

d)

60.1 amu

67.

Fluorine is added to city water supplies in the proportion of about one part per million to help prevent tooth decay. Several fluoride compounds are added to toothpaste, also to help prevent tooth decay. What is the molar mass of fluorine gas?

a)

18.998 amu

b)

38 amu

c)

9 amu

d)

18 amu

68.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
69.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
70.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
71.
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
72.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
73.

How many grams are in 7.8 moles of NaCl?

a)

476 grams

b)

460 grams

c)

452 grams

d)

462 grams

74.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
75.
What is the mole to mole ratio of propane to carbon dioxide in the equation?
a)
1:3
b)
1:5
c)
1:4
d)
1:1
76.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
77.
The first step in stoichiometry is to
a)
Determine a balanced equation
b)
convert grams to moles
c)
convert grams to liters
d)
use the mole ratio
78.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
79.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
80.
How many grams is 1.2 moles of Neon?
a)
0.05 grams
b)
16.6 grams
c)
21.2 grams
d)
24 grams
81.
How many grams are in 5.6 moles of sodium bromide?
a)
36.8 g/mol
b)
18.4 g
c)
576 g/mol
d)
576 g
82.
Convert 28.0 grams of O2 to moles.
a)
1.14 moles
b)
1.75 moles
c)
0.571 moles
d)
0.875 moles
83.
Change 7.00 moles of Na2SO4 into grams.
a)
20.3 grams
b)
994 grams
c)
770 grams
d)
0.0493 grams
84.
How many molecules are in 9.4 moles of AlCl3?
a)
5.66
b)
5.66x1024
c)
0.705
d)
1.25x1023
85.
How many moles are in 16.94g of H2O?
a)
16.94
b)
0.9403
c)
305.2
d)
1.063
86.
How many total molecules are there in 2HNO3?
a)
2
b)
6
c)
8
d)
10
87.

Determine the number of moles of AlNO3 that are in 264 g of the compound.

a)

2.97 mol

b)

3.45 mol

c)

2.73 mol

d)

1.86 mol

88.

Determine the amount of moles in CuBr that are in 276.9 g of the compound.

a)

3.2 mol

b)

1.7 mol

c)

2.1 mol

d)

1.9 mol

89.

Find the mass of 5.82 mol of MgCl2. Round to the nearest tenth.

a)

552.9 g

b)

436.8 g

c)

55.2 g

d)

555.9 g

90.

Determine the amount of moles of BaCl2 that are in 436 g of the compound.

a)

3.5 mol

b)

2.1 mol

c)

4.6 mol

d)

2.7 mol

91.

Find the mass of 3.6 mol of Au.

a)

843.6 g

b)

709.2 g

c)

435.9 g

d)

196.9 g

92.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
93.

What is the formula for Boyle's Law?

a)

P1V1=P2V2

b)

P1V1/P2V2

c)

P1V2=P2V1

d)

P1/V1=P2/V2

94.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
95.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
96.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
97.

IF we are using Boyles' law and our Pressure goes UP, what must our volume do?

a)

Go UP

b)

Go DOWN

c)

Stay the same

d)

Wrong law.

98.

Which best explains why increasing the pressure on a gas decreases the volume of the gas sample?

a)

Increasing the pressure causes the gas particles to hit the container walls more often.

b)

Increasing the pressure on a gas sample moves the gas particles closer together.

c)

Increasing the pressure on a gas sample causes the kinetic energy to increase.

99.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
100.
What is the variable for this number 32oC
a)
P
b)
T
c)
n
d)
V
101.
What is the variable for this number 9.10 atm
a)
P
b)
T
c)
n
d)
V
102.
What is the variable for this number 1.5 mol
a)
P
b)
T
c)
n
d)
V
103.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
104.
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
105.
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 
106.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

107.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
108.

At constant pressure, a balloon's volume changed from 15L to 45L. If the final temperature was 350K, what was the initial temperature?

a)

2 K

b)

1050 K

c)

117 K

d)

not enough information

109.
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
110.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
111.

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

112.

Mg3N2 + 3H2O ––> 3 MgO + 2NH3

If 10.3 g of magnesium nitride is used, what volume of ammonia gas would be collected at 20˚C and 0.989 atm?

a)

4.9 L NH3

b)

4.96 L NH3

c)

0.261 L NH3

d)

0.26 L NH3

113.

2CO + O2 −-> 2CO2

How many liters of carbon monoxide at 25.0oC and 8.56 mmHg are needed to react with 12.30 L of oxygen gas at STP?

a)

3.14 L

b)

318 L

c)

2390 L

d)

200 L

114.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
115.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
116.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
117.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
118.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
119.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams

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