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AP Chemistry Gas and Stoichiometry Review

Total questions: 145

Worksheet time: 18hrs 15mins

Name
Class
Date
1.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
2.
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
3.
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
4.
What is the measured amount of a product obtained from a chemical reaction?
a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
5.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
6.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
7.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
8.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
9.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
10.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
11.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
12.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
13.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
14.
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%
15.
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
16.
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
17.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Avogadro's Number
18.
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
19.

Determine the % composition of Potassium in the following copound KMnO4

a)

14.8%

b)

34.8%

c)

24.7%

d)

40.5%

20.

Determine the mass of calcium hydroxide produced when calcium carbide reacts with 0.64g of water according ot the following equation

CaC2 + 2H2O --> Ca(OH)2 + C2H2

a)

10.31 g Ca(OH)2

b)

41.31 g Ca(OH)2

c)

1.31 g Ca(OH)2

d)

31 g Ca(OH)2

21.

Determine the mass of lithium hydroxide produced when 0.38g of lithium nitride reacts with water according to the following equation

Li3N + 3H2O --> NH3 + 3LiOH

a)

11.78 g LiOH

b)

0.78 g LiOH

c)

12.78 g LiOH

d)

21.78 g LiOH

22.

How many moles of nitrogen gas are in 135 L of nitrogen gas at Standard Temperature and Pressure (STP)?

a)

9.64 moles of N2

b)

5.53 moles of N2

c)

6.02 moles of N2

d)

4.82 moles of N2

23.

A compound is 64.9% carbon, 13.5% hydrogen, and 21.6% oxygen. Its molecular mass is 74 g/mol. What is its molecular formula?

a)

C4H10O

b)

C5H10

c)

C2H4O2

d)

None of these

24.

Four students tried to balance the following Reaction:


Mg + Fe2O3 → MgO + Fe


Which student is correct?

a)

3Mg + Fe2O3 → 3MgO + 2Fe

b)

Mg + Fe2O3 → MgO3+ Fe2

c)

2Mg + Fe2O2 → 2MgO + 2Fe

d)

3Mg + 2Fe2O3 → 3MgO + 2Fe

25.
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
26.
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
27.

2Al + 3H2SO4 -> Al2(SO4)3 + 3H2How 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

28.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
29.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
30.
What is the name of FeSO4?
a)
Iron Sulfite
b)
Iron (II) Sulfite
c)
Iron(IV) Sulfate
d)
Iron (II) Sulfate
31.
what is the name of CCl4?
a)
carbon tetrachloride
b)
monocarbon tetrachloride
c)
tetracarbon monochloride
d)
carbon chloride
32.
calcium oxide
a)
Ca2O2
b)
Ca2O
c)
CaO
d)
CaO2
33.
Find the percentage composition of  Mg in Mg3(PO4)2.
   

a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
34.
What is the percentage of chromium in K2Cr2O7?
a)
38.1%
b)
27.2%
c)
34.7%
d)
100%
35.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
36.
A hydrate of magnesium chloride is present and the following data is collected:
mass of crucible = 22.130 grams
mass of crucible + hydrate = 25.290 grams
mass of crucible and contents after heating = 23.491 grams
What is the complete formula of this hydrate?
a)
MgCl2 · 7H2O
b)
MgCl2 · 11H2O
c)
MgCl2 · 6H2O
d)
MgCl2 · 13H2O
37.
In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulphuric acid. The solid line on the graph shows the volume of gas given off when the 2 g lump is used. Which dotted line is obtained when the zinc is powdered? 
a)
A
b)
B
c)
C
d)
D
38.
Calcium carbonate reacts with hydrochloric acid to form carbon dioxide. Which changes would slow this reaction down?
 1  decreasing the concentration of hydrochloric acid
 2  decreasing the particle size of calcium carbonate
3  decreasing the temperature 
a)
1 and 2 only 
b)
1 and 3 only 
c)
2 and 3 only 
d)
1, 2 and 3 
39.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
40.
Determine the molar mass for CCl4
a)
153.8 g/mol
b)
47.54 g/mol
c)
189.35 g/mol
d)
82.9 g/mol
41.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
42.
Determine the amount of moles in 1.50 x 1023 atoms of fluorine.
a)
9.03 x 1046 moles
b)
0.249 moles
c)
4.73 moles
d)
0.0131 moles
43.
Determine the number of
atoms in
2.50 moles of zinc.
a)
1.51 x 1024 atoms
b)
4.15 x 10-24 atoms
c)
2.71 x 10-22 atoms
d)
163 atoms
44.
Find the Molar Mass of:
Ga2(SO3)3
a)
280 g/mol
b)
400 g/mol
c)
380 g/mol
d)
480 g/mol
45.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
46.
A student is studying the effect of temperature on the speed of a reaction between hydrochloric acid and magnesium ribbon. What is the independent variable in her experiment?
a)
Hydrochloric acid
b)
Speed
c)
Temperature
d)
How fine is the magnesium ribbon
47.

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

48.

A 2.00-liter sample of nitrogen gas at 27° C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is

a)

68o C

b)

120o C

c)

477o C

d)

677o C

49.

A sample of 0.010 mole of oxygen gas is confined at 127°C and 0.80 atmosphere. What would be the pressure of this sample at 27°C and the same volume?

a)

0.10 atm

b)

0.20 atm

c)

0.60 atm

d)

0.80 atm

50.

Samples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound?

a)

XeF

b)

XeF3

c)

XeF4

d)

XeF6

51.

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)

52.

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

53.

A sample of 9.00 grams of aluminum metal is added to an excess of hydrochloric acid. The volume of hydrogen gas produced at standard temperature and pressure is

a)

22.4 Liters

b)

11.2 Liters

c)

7.46 Liters

d)

5.60 Liters

54.

An excess of Mg(s) is added to 100. mL of 0.400 M HCl. At 0ºC and 1 atm pressure, what volume of H2 gas can be obtained?

a)

22.4 mL

b)

44.8 mL

c)

224 mL

d)

448 mL

55.

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

56.

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

57.

At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion?

a)

CO and CO2

b)

CO and N2

c)

NO2 and N2O4

d)

N2O and NO2

e)

N2 and O2

58.

Convert 191 atm to kPa.

a)

194 kPa

b)

1.94 x 104 kPa

c)

25.5 kPa

d)

1.89 kPa

e)

45600 kPa

59.

Convert 191 mmHg to atm.

a)

145000 atm

b)

0.251 atm

c)

890 atm

d)

3.55 atm

e)

1.23 x 103 atm

60.
If the temperature of a gas increase, the pressure...
a)
Decreases
b)
Increases
c)
Does not change
61.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
62.

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

63.
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 
64.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
65.

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.

66.

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

67.

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

68.

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

69.

Mg3N2 + 3H2O ––> 3 MgO + 2NH3

If 10.3 L of ammonia gas at 20.0˚C and 0.989 atm is created, how many liters of water at STP are required?

a)

0.423 L H2O

b)

14.2 L H2O

c)

0.204 L H2O

d)

10.3 L H2O

70.

2CO + O2 −-> 2CO2

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

0.0199

71.

4NH3+6NO --> 5N2 + 6H2O

How many liters of NH3 at 32.6 oC and 4.25 kPa are needed to react completely with 30.0L of NO at STP?

a)

5.27 L

b)

534 L

c)

5.2 L

d)

533.6 L

72.

When solving for gas stoichiometry problems which of the following is correctly matched?

a)

STP conditions; molar mass

b)

NON STP conditions; PV=nRT

c)

STP conditions; PV=nRT

d)

NON STP conditions; 22.4 moles

73.

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

74.

2NaN3 → 2Na + 3N2

At what pressure(atm) is the nitrogen gas sample that is collected when 48.4 g of NaN3 decomposes? The temperature of the gas is 25.0°C and the volume is 18.4 L.

a)

151 atm

b)

1130 atm

c)

0.125 atm

d)

1.48 atm

75.

2Cu2S + 3O2 → 2Cu2O + 2SO2

This reaction uses 18.2 g of copper (I) sulfide. What volume of sulfur dioxide gas would be collected at 237°C and 10.7 atm?

a)

0.446 L

b)

57 L

c)

0.207 L

d)

0.21 L

76.

Assume that 5.6 L H2 at STP reacts with excess CuO according to the following equation:

CuO (s) + H2 (g) ---> Cu (aq) + H2O (l)


How many moles of Cu are produced?

a)

0.250 mol

b)

2.50 mol

c)

25.0 mol

d)

25.00000 mol

77.
You have 3.5 L of H2 (g) at STP. How many moles of gas are there?
a)
22.4 mol
b)
22.4 L
c)
0.16 mol
d)
0.16 L
78.

How many liters of NH3 are needed to react completely with 30.0L of NO?

4NH3(g) + 6NO (l)--> 5N2 (g) + 6H2O (l)

a)

5.0 L

b)

20.0 L

c)

7.5 L

d)

120.0 L

79.

Which mole ratio is correct for the given chemical equation?


2N2 (g) + 5O2 (g) -----> 2N2O5 (g)

a)

2 mol N2 to 5 mol N2O5

b)

2 mol N2 to 2 mol N2O5

c)

5 mol O2 to 2 mol NO2

d)

None are correct.

80.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
81.

2CO (g) + O2 (g) --> 2CO2 (g)

How many liters of carbon dioxide (CO2) are produced from 10L of carbon monoxide (CO)?

a)

10

b)

20

c)

1

d)

5

82.

What volume of hydrogen(H2) will be produced at STP by the reaction 67.3 g of magnesium with excess water according to the following reaction?

1Mg (s) + 2H2O (l) --> Mg(OH)2 (aq) + H2 (g)

a)

62L

b)

65L

c)

31L

d)

124L

83.

Solid aluminum react with HCl according to the following balanced equation at STP:

2Al (s) + 6HCl (aq) --> 2AlCl3 (aq) + 3H2 (g)


If 13.5 g of Al (s) reacts with excess HCl, how many liters of H2 gas are generated?

a)

15.2 L

b)

16.8 L

c)

12.5 L

d)

14.8 L

84.

How do I change from moles to liters in STP?

a)

divide by 22.4

b)

multiple by Avo number

c)

multiply by 22.4

d)

multiply by molar mass

85.
How do I move from grams to moles
a)
multiply by molar mass
b)
divide by molar mass
c)
multiply by Avo number
d)
divided by Avo number
86.
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
87.
You have 3.5 L of H2 (g) at STP. How many moles of gas are there?
a)
22.4 mol
b)
22.4 L
c)
0.16 mol
d)
0.16 L
88.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
89.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
90.
What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium with excfess water according to the following reaction?
1Mg + 2H2O --> Mg(OH)2 + H2
a)
62L
b)
65L
c)
31L
d)
124L
91.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
92.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
93.
How do gas molecules move?
a)
In an orderly fashion
b)
Constantly and randomly
c)
In straight-line paths
d)
In a circular motion
94.
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
95.
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
96.
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)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
97.
A sample of oxygen at 28.0°C has 340.0 kPa. What will its temperature be at 150.0 kPa?
a)
132.8 K
b)
132.8 °C
c)
682.2 K
d)
12.35 K
98.
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)
57.5 °C
b)
57.5 °K
c)
330.5 K
d)
330.5°C
99.
f a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?
a)
9 L
b)
.69 L
c)
1.44 L
100.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
101.

A water bottle at STP is cooled to -155°C. What is the new pressure?

a)

3.2 atm

b)

0.43 atm

c)

1.8 atm

d)

0.27 atm

102.

The pressure of a 6.5 L sample of oxygen gas is measured to be 3.8 atm. If the gas is transferred into a 12 L tank, what is the new pressure?

a)

6.6 atm

b)

3.9 atm

c)

4.5 atm

d)

2.1 atm

103.

A student transfers a gas at STP from a 11.0 L tank to a 25.0 L tank. If the pressure remains constant, what is the new temperature?

a)

620 K

b)

393 K

c)

254 K

d)

530 K

104.

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)

2.1 atm

c)

1.6 atm

d)

3.4 atm

105.

A sample of gas containing 9.2 moles is transferred from an 13 L tank to a 23 L tank. What is the new number of moles that can be stored in the tank?

a)

10.2 mol

b)

13.7 mol

c)

19.1 mol

d)

16.3 mol

106.

A student places four gases into a container. The pressures of the gases are: N2=2.1 atm, H2=1.3 atm, He=1.9 atm & Ar=3.4 atm. What is the total pressure?

a)

5.1 atm

b)

8.7 atm

c)

7.4 atm

d)

6.9 atm

107.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

108.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
109.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
110.
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)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
111.
Three gases, Ar, N2 and H2 are mixed in a sealed container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
112.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K
113.
A gas of volume V is placed in a balloon.  Determine the new volume of the balloon if the pressure is tripled. The new volume will be ____ what it was originally.  
a)
1/3 of
b)
1/6 of
c)
1/9 of
d)
 9 times
114.
A gas of volume V is placed in a balloon. The absolute (Kelvin) temperature is tripled. The volume will be _____ what it was originally. 
a)
1/3
b)
1/6
c)
3 times
d)
6 times
115.
A gas of volume V is place in a balloon. The pressure is reduced to 1/5 of the original pressure. The volume will be _____ what it was originally.  
a)
the same as 
b)
1/5
c)
9 times
d)
5 times
116.
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
117.
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
118.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
119.
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
120.
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 
121.
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
122.
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 
123.
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
124.
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
125.
What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?
a)
3670 atm
b)
0.245 atm
c)
4.08 atm
d)
605 atm
126.
At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?
a)
22.9 Liters
b)
2355 Liters
c)
0.0630 Liters
d)
15.9 Liters
127.
An 18 liter container holds 16.00 grams of oxygen gas (O2) at 45 °C. What is the pressure in the container?
a)
0.725 atm
b)
11.0 atm
c)
23.2 atm
d)
1.45 atm
128.

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

129.

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

130.

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

131.

Mg3N2 + 3H2O ––> 3 MgO + 2NH3

If 10.3 L of ammonia gas at 20.0˚C and 0.989 atm is created, how many liters of water at STP are required?

a)

0.423 L H2O

b)

14.2 L H2O

c)

0.204 L H2O

d)

10.3 L H2O

132.

2CO + O2 −-> 2CO2

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

0.0199

133.

4NH3+6NO --> 5N2 + 6H2O

How many liters of NH3 at 32.6 oC and 4.25 kPa are needed to react completely with 30.0L of NO at STP?

a)

5.27 L

b)

534 L

c)

5.2 L

d)

533.6 L

134.

When solving for gas stoichiometry problems which of the following is correctly matched?

a)

STP conditions; molar mass

b)

NON STP conditions; PV=nRT

c)

STP conditions; PV=nRT

d)

NON STP conditions; 22.4 moles

135.

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

136.

2NaN3 → 2Na + 3N2

At what pressure(atm) is the nitrogen gas sample that is collected when 48.4 g of NaN3 decomposes? The temperature of the gas is 25.0°C and the volume is 18.4 L.

a)

151 atm

b)

1130 atm

c)

0.125 atm

d)

1.48 atm

137.

2Cu2S + 3O2 → 2Cu2O + 2SO2

This reaction uses 18.2 g of copper (I) sulfide. What volume of sulfur dioxide gas would be collected at 237°C and 10.7 atm?

a)

0.446 L

b)

57 L

c)

0.207 L

d)

0.21 L

138.

Assume that 5.6 L H2 at STP reacts with excess CuO according to the following equation:

CuO (s) + H2 (g) ---> Cu (aq) + H2O (l)


How many moles of Cu are produced?

a)

0.250 mol

b)

2.50 mol

c)

25.0 mol

d)

25.00000 mol

139.
You have 3.5 L of H2 (g) at STP. How many moles of gas are there?
a)
22.4 mol
b)
22.4 L
c)
0.16 mol
d)
0.16 L
140.

How many liters of NH3 are needed to react completely with 30.0L of NO?

4NH3(g) + 6NO (l)--> 5N2 (g) + 6H2O (l)

a)

5.0 L

b)

20.0 L

c)

7.5 L

d)

120.0 L

141.

Which mole ratio is correct for the given chemical equation?


2N2 (g) + 5O2 (g) -----> 2N2O5 (g)

a)

2 mol N2 to 5 mol N2O5

b)

2 mol N2 to 2 mol N2O5

c)

5 mol O2 to 2 mol NO2

d)

None are correct.

142.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
143.

2CO (g) + O2 (g) --> 2CO2 (g)

How many liters of carbon dioxide (CO2) are produced from 10L of carbon monoxide (CO)?

a)

10

b)

20

c)

1

d)

5

144.

What volume of hydrogen(H2) will be produced at STP by the reaction 67.3 g of magnesium with excess water according to the following reaction?

1Mg (s) + 2H2O (l) --> Mg(OH)2 (aq) + H2 (g)

a)

62L

b)

65L

c)

31L

d)

124L

145.

Solid aluminum react with HCl according to the following balanced equation at STP:

2Al (s) + 6HCl (aq) --> 2AlCl3 (aq) + 3H2 (g)


If 13.5 g of Al (s) reacts with excess HCl, how many liters of H2 gas are generated?

a)

15.2 L

b)

16.8 L

c)

12.5 L

d)

14.8 L

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