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Stoichiometry

Total questions: 114

Worksheet time: 4hrs 37mins

Name
Class
Date
1.
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
2.
11.
LiOH + KCl → LiCl + KOH 

b)  I actually produced 6 grams of lithium chloride and I began this reaction with 20 grams of lithium hydroxide. What is my percent yield?
a)
16.9%
b)
5.91%
c)
1.88%
d)
12.3%
3.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
4.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
5.
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
6.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
7.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
8.
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
9.
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
10.
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
11.
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
12.
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
13.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
14.
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
15.
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
16.
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
17.
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
18.
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
19.
 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
20.
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
21.
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
22.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
23.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
24.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
25.
What is the total number of atoms present in 5Na3PO4
a)
5
b)
40
c)
55
d)
8
26.
How many Mn atoms are found in the following compound?
3Cr(MnO4)6
a)
3
b)
4
c)
6
d)
18
27.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
28.
Is the following equation balanced?...
Al + O2 --> 2Al2O3
a)
Yes!
b)
No!
29.
Element or compound?
H2O
a)
Element
b)
Compound
30.
Element or compound?
O2
a)
Element
b)
Compound
31.
What is the number before a chemical formula called?
Ex: 2H2 + O2 --> 2H2O
a)
Coefficient
b)
Subscript
c)
Atom
d)
Equation
32.
How many aluminum atoms are in Al2(SO4)3?
a)
1
b)
2
c)
3
d)
4
33.
In which of these compounds are there twice as many oxygen atoms as hydrogen atoms?
a)
H3PO4
b)
H2SO4
c)
HClO3
d)
H2O
34.
How many atoms are in the neurotransmitter serotonin? The formula for serotonin is C10H12N2O
a)
10
b)
20
c)
25
d)
23
35.
How many atoms are in the neurotransmitter serotonin? The formula for serotonin is C10H12N2O
a)
10
b)
20
c)
25
d)
23
36.
What information could a student determine from only the chemical formula of a protein?
a)
The color of the protein
b)
The number of molecules in each sequence of the protein
c)
The physical arrangement of atoms in the structure of the protein
d)
The number of atoms of each element in the protein
37.
Is the following equation balanced?
2C2H2 + 5O2 --> 4CO2 + 2H2O
a)
yes
b)
no
38.
Is the following equation balanced?
4Fe + 3O2 --> 2Fe2O3
a)
yes
b)
no
39.
Is the following reaction balanced?
NaHCO3 --> Na2CO3 + H2O + CO2
a)
yes
b)
no
40.
Is the following reaction balanced?
2CH3OH + 3O2 --> 2CO2 + 4H2O
a)
yes
b)
no
41.
Which of the following equations are correctly balanced?
a)
12CO2 +H2O --> C6H12O6 + O2
b)
CO2 + 9H2O --> C6H12O6 + O2
c)
CO2 + H2O --> 3C6H12O6 + O2
d)
6CO2 + 6H2O --> C6H12O6 + 6O2
42.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
43.
Which of the following reactions is balanced?
a)
2CH4 + O2 -> CO2 + H2O
b)
CH4 + 2O2 -> CO2 + H2O
c)
CH4 + 2O2 -> CO2 + 2H2O
d)
None of the chemical equations are balanced.
44.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
45.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
46.
Which coefficients balance this equation:
NH3  +  O2 ---->   NO  + H2O
a)
2,3,5,6
b)
5,5,4,6
c)
4,6,4,5
d)
4,5,4,6
47.
What is the unit of measurement for the amount of a substance
a)
Volume
b)
Mass
c)
Concentration
d)
Moles
48.
What is true about the molar mass of chlorine gas?
a)
The molar mass is 35.45 g
b)
The molar mass is 70.90 g
c)
The molar mass is equal to 1 mole of chlorine atoms
d)
none of the above.
49.
What is the volume of liquid in this graduated cylinder?
a)
40.0 mL
b)
40.3 mL
c)
43.0 mL
d)
44.0 mL
50.

5,000 mg=____________grams

a)

500 grams

b)

50 grams

c)

5 grams

d)

5,000 grams

51.

4,000 grams=_____________kg

a)

40

b)

400

c)

4

d)

4,000

52.

9 g=______________mg

a)

9 mg

b)

900 mg

c)

90 mg

d)

9,000 mg

53.
CaCO3 represents a chemical
a)
Symbol
b)
Formula
c)
Subscript
d)
Reaction
54.
In balancing chemical equations, we change
a)
Coefficients
b)
Subscripts
c)
Both can be changed
d)
None can be changed
55.
How many phosphorus atoms are in PO4?
a)
1
b)
2
c)
3
d)
4
56.
How many hydrogen atoms are in 2 H2?
a)
1
b)
2
c)
3
d)
4
57.
Which number should go in the blank?
_ H2 + O2 -> 2 H2O
a)
1
b)
2
c)
3
d)
0
58.
Which number should go in the blank?
2 Na+ _ Cl2 -> 2 NaCl
a)
1
b)
2
c)
3
d)
0
59.
Which number should go in the blank?
Mn + _ HNO3 → Mn(NO3)2 + H2
a)
1
b)
2
c)
3
d)
0
60.
Which number should go in the blank?
Al(NO3)3 + _  NaOH -> Al(OH)3 + 3 NaNO3
a)
1
b)
2
c)
3
d)
0
61.
Which number should go in the blank?
Al(NO3)3 + _  NaOH -> Al(OH)3 + 3 NaNO3
a)
1
b)
2
c)
3
d)
0
62.
How many oxygen atoms are present in the following? 
4Ca(OH)2
a)
4
b)
6
c)
8
d)
1
63.
How many Iron (Fe) atoms are in this chemical formula?
a)
2 iron atoms
b)
6 iron atoms
c)
5 iron atoms
d)
4 iron atoms
64.

What physical state symbol should be included for carbon dioxide?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

65.

What physical state symbol should be included for glucose?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

66.

What physical state symbol should be included for oxygen?

a)

(s) - solid

b)

(l) - liquid

c)

(g) - gas

d)

(aq) - aqueous

67.

Why does oxygen's symbol have a subscript "2"?

a)

Because it is monoatomic.

b)

Because it is diatomic.

c)

Because it is triatomic.

68.

A mole in chemistry is a counting unit.

a)

True

b)

False

c)

Unsure

69.

One mole of water & one mole of glucose contain the same number of molecules.

a)

True

b)

False

c)

Unsure

70.

One mole of H2 contains the same number of atoms as one mole of CO2.

a)

True

b)

False

c)

Unsure

71.

Avogadro’s constant is:

a)

6.02 x 1022

b)

6

c)

6.02 x 1023

d)

3.01 x 1023

72.

How much would 1 mole of carbon weigh? The relative molecular weight of carbon is 12.

a)

12 g

b)

24 g

c)

48 g

d)

96 g

73.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
74.
How many potatoes are in one dozen potatoes?
a)
10
b)
12
c)
2
d)
6.02 x 1023
75.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
76.
We use the periodic table to calculate...
a)
mass
b)
molar mass
c)
moles
77.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
78.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
79.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
80.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
81.
Which one is empirical?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
82.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
83.
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
84.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
85.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
86.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

87.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
88.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
89.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

90.

2.40 g of an explosive, J, contains 0.473 g of nitrogen. J also contains 33.8% carbon and 1.41% hydrogen by mass. The remainder of J is oxygen.


What is the empirical formula of J?

a)

C4HNO2

b)

CH2N2O

c)

C2HNO2

d)

CHNO

91.
In which compound is the percent composition by mass of Cl equal to 42%?
a)
HClO (gram formula mass = 52 g/mol)
b)
HClO2 (gram formula mass = 68 g/mol)
c)
HClO3 (gram formula mass = 84 g/mol)
d)
HClO4 (gram formula mass = 100 g/mol)
92.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
93.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

94.

How many moles are in 19.82 g Mg?

a)

1.23 mol Mg

b)

481.70 mol Mg

c)

1.00 mol Mg

d)

0.82 mol Mg

95.

How many moles are in 3.01 x 1022 atoms of magnesium?

a)

0.05 moles

b)

1.81 x 1046 moles

c)

5.00 x 1021 moles

d)

5.00 moles

96.

How many grams are in 1.2 x 1024 atoms of C?

a)

29.34 grams

b)

23.94 grams

c)

6.02 grams

d)

1.21 grams

97.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

98.
Calculate the number of atoms in 0.0340 g Zn.
a)
5.200 x 10-4 atoms Zn
b)
3.130 x 1023 atoms Zn
c)
3.130 x 1020 atoms Zn
d)
1 atom Zn
99.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
100.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
101.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
102.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
103.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
104.

What is the empirical formula for the following:

32.40% sodium, 22.5% sulfur; 45.1 % oxygen, 37.75% water?

a)

Na2SO4H6O3

b)

Na2SO4 * 2H2O

c)

Na2SO4 * 3H2O

d)

Na2SO4 * (H2O)

105.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
106.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
107.

Which of the following is a covalent bonding?

a)

MgS

b)

NaCl

c)

CH4

d)

LiBr

108.

Which of the following is a non-polar covalent bonding?

a)

Carbon Dioxide

b)

Oxygen gas

c)

Ammonia

d)

Water

109.

What characteristic differentiates covalent bonding from ionic bonding?

a)

Electrons are transferred from one atom to another to form a bond

b)

Electrons are shared in pairs from one atom to another to form a bond

110.

Which of the following is a non-polar covalent bonding?

a)

Carbon Dioxide

b)

Oxygen gas

c)

Ammonia

d)

Water

111.

What characteristic differentiates covalent bonding from ionic bonding?

a)

Electrons are transferred from one atom to another to form a bond

b)

Electrons are shared in pairs from one atom to another to form a bond

112.

Which of the following is NOT a polar covalent bonding?

a)

H2

b)

CH4

c)

CO2

d)

SO2

113.

Which of the following is a characteristic of a covalent bonding?

a)

Crystalline solids

b)

High melting point

c)

Transfer electrons

d)

Low electrical conductor

114.

What is the difference in electronegativity value of carbon dioxide?

a)

0.10

b)

0.9

c)

0.8

d)

0.7

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