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Stoichiometry Review (A and B)

Total questions: 81

Worksheet time: 4hrs 13mins

Name
Class
Date
1.

CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was used in the above reaction. Calculate the moles of H2O that will be produced?

a)

3 moles

b)

66 grams

c)

1.5 mol

d)

8.72 moles

2.

2Fe2O3 + 3C → 4Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 81.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

79.14%

3.
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%
4.

N2 + 3H2 → 2NH3

What is the mole ratio between Nitrogen and Ammonium in the above reaction?

a)

1 moles NH3 / 2 moles N2

b)

2 moles NH3 / 1 moles N2

c)

2 moles N2 / 3 moles NH3

d)

1 moles N2 / 3 moles NH3

5.

In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

4:3

d)

2:3

6.

4NH3 + 5O2-->4NO + 6H2O

What is the total number of moles of NO produced when 1 mole of O2 is completely consumed?

a)

1

b)

1.2

c)

0.8

d)

4

7.

6CO2 + 6H2O --> C6H12O6 + 6O2

What is the total number of moles of water needed to make 2.5 moles of C6H12O6?

a)

2.5

b)

6

c)

12

d)

15

8.

How many moles is 100 grams of FeCl2?

a)

0.79 moles

b)

100 moles

c)

126.745 moles

d)

7.9 moles

9.

What is Avegadro's number?

a)

1 mole

b)

6.02 X 1023

c)

1 gram

d)

10 m

10.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: If 16 moles of carbon dioxide are formed by this reaction, how many moles of water were also produced?

a)

4 mol H2O

b)

6 mol H2O

c)

24 mol H2O

d)

96 mol H2O

11.

CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. How many grams of Co2 will be formed?

a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
12.

Molecular Formula = C2F6

Choose the correct empirical formula.

a)

CF

b)

C2F6

c)

C3F

d)

CF3

13.

Empirical Formula = CF2

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

14.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
15.

10. How many moles are in 89 grams of copper (II) hydroxide, Cu(OH)2?

4 lines
16.

The empirical formula must be lowest whole number ratio.

a)

True

b)

False

17.

How many atoms would be contained in 454 grams of iron?

a)

6.02 x 1023 atoms

b)

8.14 atoms

c)

4.89 x 1024 atoms

d)

55.9 x 1023 atoms

18.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of oxygen?

a)

29%

b)

43%

c)

57%

d)

73%

19.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of bromine? Hint - consider the mass of both atoms of bromine in your calculation.

a)

13%

b)

43%

c)

63%

d)

87%

20.
N2 + 3H2 --> 2NH3
What is the total number of moles of NH3 produced when 10 moles of H2 reacts completely with N2?
a)
6.7
b)
2.0
c)
3.0
d)
15.0
21.
H2+Cl2-->2HCl
How many moles of Cl2 is needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
22.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of NO produced when 1 mole of O2 is completely consumed?
a)
1
b)
1.2
c)
0.8
d)
4
23.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
24.
N2 + 3H2 --> 2NH3
How many moles of N2 is needed to react with 6 moles of H2?
a)
6.7
b)
2.0
c)
3.0
d)
15.0
25.

Which of the following represent a mole ratio between silver nitrate (AgNO3) and copper(II) nitrate (Cu(NO3)2) in the following reaction: 2AgNO3 + Cu --> Cu(NO3)2 + 2Ag

a)
2 mol AgNO3 / 2 mol Ag
b)
2 mol Ag / 2 mol AgNO3 
c)
2 mol AgNO3 / 2 mol Cu(NO3)2
d)
2 mol AgNO3 / 1 mol Cu(NO3)2
26.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of carbon dioxide to water?

a)
b)
c)
d)
27.

What number should be in front of each substance in the chemical equation?

___N2+___F2 --> ___ NF3

a)

1, 2, 3

b)

2, 1, 3

c)

1, 3, 2

d)

3, 1, 2

28.

Where are the numbers for a mole ratio found?

a)

They are part of the chemical formulas for the reactants / products.

b)

They are given in the problem.

c)

They are found on the periodic table for those elements.

d)

They are found as coefficients in the reaction's balanced chemical equation.

29.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: How many moles of ethane (C2H6) are required to produce 13.5 moles of water from the above reaction?

a)

4.5 mol C2H6

b)

27 mol C2H6

c)

40.5 mol C2H6

d)

81 mol C2H6

e)

162 mol C2H6

30.

What is the mole ratio of Mg to MgCl2? HINT: Balance the equation first.

Mg(s) + HCl(aq) → MgCl2(aq) + H2(g)

a)

2 mol Mg/ 1 mol MgCl2

b)

1 mol Mg/ 2 mol MgCl2

c)

1 mol Mg/ 1 mol MgCl2

d)

2 mol Mg/ 2 mol MgCl2

31.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
32.

In the balanced equation 2Al2O3 → 4Al + 3O2, what is the mole ratio of aluminum to oxygen?

a)

3 : 2

b)

3 : 4

c)

4 : 3

d)

2 : 3

33.

3Mg + Fe2O3 → 3MgO + 2Fe

What is the mole ratio of magnesium to iron?

a)

3 : 2

b)

2 : 3

c)

1 : 2

d)

3 : 1

34.

How many step will it take for me to go from moles given to moles unknown?

a)

1

b)

2

c)

3

d)

4

35.

How many steps will it take me to go from grams to grams?

a)

4

b)

3

c)

2

d)

1

36.
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
37.

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

38.

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

39.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

40.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
41.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
42.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

43.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

44.

What is the mass of 2.50 mole of oxygen gas O2?

a)

40 g

b)

80 g

c)

16 g

d)

32 g

45.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)

44.01 moles

b)

1421.52 moles

c)

32.3 moles

d)

0.73 moles

46.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
47.
How many atoms are in 1 mole of NaCl? 
a)
6.02 x 1023
b)
58 
c)
11
d)
17
48.
How are the mole and atomic masses of elements related?  
a)
The atomic mass of any substance is always equal to 1 mole of that substance 
b)
The atomic mass added up with itself by 6.02 x 1023 equals the amount of atoms
c)
The atomic mass is the amount of protons plus number of atoms
d)
Atoms combined make up molecules, which are the measurement of atomic masses 
49.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

50.

At STP, 1 mol of gas has a volume of

a)

34L

b)

22.4L

c)

60L

d)

0.6L

51.

Determine the volume, in liters, of 1.2 mole SO2 gas at STP.

a)

13 L

b)

26 L

c)

6.5 L

52.

Match the following units to their correct category.

a)

Grams

1.

Mass

b)

Liters at STP

2.

Volume

c)

Units, Atomes, Molecules

3.

Particles

53.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

392.6 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

54.
How many moles of magnesium are in 3.01x1022 atoms of magnesium?
a)
5.00x1044 moles Mg
b)
0.050 moles Mg
c)
1.81x1046 moles Mg
d)
5 moles Mg
55.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
1.25 molec AlCl3
d)
1.25x1023 molec AlCl3
56.
Convert 28.0 grams of O2 to moles.
a)
1.14 moles
b)
1.75 moles
c)
0.571 moles
d)
0.875 moles
57.
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
58.
Change 7.00 moles of Na2SO4 into grams.
a)
20.3 grams
b)
994 grams
c)
770 grams
d)
0.0493 grams
59.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
60.

Which choice is the fromula for calculating percent by mass?

a)

a

b)

b

c)

c

d)

d

61.
a)

16.00

b)

1.01

c)

17.01

d)

18.02

62.

a)

5.60%

b)

11.20%

c)

88.79%

d)

18.02%

63.

a)

5.60%

b)

11.20%

c)

88.79%

d)

18.02%

64.

a)

28.01

b)

58.93

c)

117.86

d)

44.01

65.

a)

27.29%

b)

36.35%

c)

72.27%

d)

1.34%

66.

a)

27.29%

b)

36.35%

c)

72.27%

d)

1.34%

67.

a)

201.25

b)

84.32

c)

52.32

d)

36.32

68.

a)

56.93%

b)

28.83%

c)

14.24%

d)

18.98%

69.

a)

56.93%

b)

28.83%

c)

14.24%

d)

18.98%

70.

a)

56.93%

b)

28.83%

c)

14.24%

d)

18.98%

71.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
72.

Molecular Formula = C2F6

Choose the correct empirical formula.

a)

CF

b)

C2F6

c)

C3F

d)

CF3

73.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
74.

Empirical Formula = CF2

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

75.

Molecular Formula = Si2F6

Choose the correct empirical formula.

a)

SiF

b)

Si2F6

c)

SiF3

d)

Si4F12

76.

How would you calculate the molar mass for C4H6?

a)

12.0111 + 1.00794

b)

4(12.0111) + 6(1.00794)

c)

2(12.0111) + 3(1.00794)

d)

6(12.0111) + 4(1.00794)

77.

The empirical formula of a substance is CH2O. The molar mass is 180g/mol. What is the molecular formula?

a)

CH2O

b)

C3H6O3

c)

C6H12O6

d)

C12H6O12

78.

What is the empirical formula of K2SO4?

a)

K2SO4

b)

KSO2

c)

K2SO2

d)

KSO8

79.

What is the empirical formula if you have 81.7% carbon and 18.3% hydrogen?

a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
80.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
81.

A chemical formula that shows the smallest whole number ratio of the elements / atoms_________

a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula

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