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Chapter 3 Review--Chem II

Total questions: 100

Worksheet time: 3hrs 28mins

Name
Class
Date
1.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
d)
Left side is balanced
2.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
3.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
4.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
5.

How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3

(a)  

6.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
7.
Name the part in red:

_2_H2 + _1_O2 -> _2_H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
8.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Reactant
d)
Subscript
9.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Reactant
d)
Subscript
10.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
11.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
12.

How many O's are in Al₂(SO₄)₃

(a)  

13.

How many H's are found in 3(NH₄)₂CrO₄

a)

4

b)

2

c)

8

d)

24

14.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

15.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

16.

Examine the following chemical equation, which shows only the reactants and one product.


Zn + 2HCl ➡️ ZnCl2 + ?


How many H atoms must be present in the second product that is formed?

a)

1

b)

2

c)

3

d)

4

17.

Which of the following equations does not demonstrate the law of conservation of mass?

a)

2Na + Cl2 ➡️ 2NaCl

b)

NaOH + HCl ➡️ NaCl + H20

c)

P4 + 5O2 ➡️ 2P4O10

18.

What is the empirical formula for the following molecular formula: C6H14

a)

C6H14

b)

C3H7

c)

CH2

d)

CH3

19.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180?

a)

CH2O

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

20.

What is the molecular formula of a compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole?

(a)  

21.

What is the empirical formula for the following molecular formula: C5H12

a)

C5H12

b)

CH3

c)

CH2

d)

C2.5H6

22.

The empirical formula for Caffeine (C8H10N4O2) is:

a)

C5H5N2O

b)

C4H5N2O

c)

C4H5NO

d)

C4H5NO2

23.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
24.
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
25.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
26.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

27.

Calculate the molar mass of Barium Acetate

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

28.

Calculate the molar mass of Cuprous Oxide

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

29.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

30.

What percentage of the total atomic mass of carbon monoxide is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

31.

Calculate the percentage by mass of oxygen in calcium carbonate. Give the answer to 1 decimal place.

Relative atomic masses: Ca = 40 C = 12 O = 16



(a)  

32.

Calculate the percentage by mass of nitrogen in potassium nitrate. Give the answer to 1 decimal place.

Relative atomic masses: K = 39 N = 14 O = 16



(a)  

33.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
34.

What percentage of the total atomic mass of magnesium bromide is composed of magnesium?

(a)  

35.

What is the percent composition of benzene, C6H6?

a)

C = 50.%

H = 50.%

b)

C = 85.7 %

H = 14.3%

c)

C = 92.2%

H = 7.8%

d)

C = 71.9%

H = 28.1%

36.

Find the mass of 11.37 mol of BaO. Round to the nearest whole number.

a)

1,354 g

b)

1,740 g

c)

17.40 g

d)

1,684 g

37.

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

38.

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

a)

554.1 g

b)

436.8 g

c)

55.2 g

d)

555.9 g

39.

What is the mass of 0.750 moles of (NH4)3PO4?

a)

110 g

b)

121.75 g

c)

111.75 g

d)

112 g

40.

What is the mass of 0.75 moles of (NH4)3PO4?

a)

0.0044 g

b)

110 g

c)

74 mole

d)

91 g

e)

25 mole

41.

How many moles are 454 grams of iron (Fe)?

a)

25,333 moles

b)

398.2 moles

c)

8.14 moles

d)

814 g

e)

456 moles

42.

Which has a larger molar mass in one mole: Al or Cl?

a)

Al

b)

Cl

c)

they're the same

d)

You can't guess that without more information

43.

How many moles of water are there in 24.3g of water?

a)

2.16 mol

b)

1.35 mol

c)

3.35 g

d)

1.65 mol/g

e)

2.16 g/mol

44.
How many grams are in 7.5 X 1023 molecules of H2SO4
a)

98.09 g H2SO4

b)

120g H2SO4

c)

45g H2SO4

d)

122g H2SO4

45.

When you are solving for molecules, atoms, and particles you always use what number?

a)

6.02 X 1023

b)

Lucky 7

c)

Guess

d)

24

46.

How many moles are in 2.85 x 1018 atoms of iron, Fe?

a)

41.4 molecules

b)

4.14 x 1023 molecules

c)

4.14 x 1025 molecules

d)

1.83 x 10-21 molecules

47.
How many grams are in 3.3 x1023 molecules of N2I3
a)

126g

b)

260g

c)

790.g

d)

220g

48.
How many grams are in 7.4 X 1023 molecules of AgNO3
a)

69g

b)

698g

c)

209g

d)

210g

49.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
50.
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
51.
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
52.

Which molecular formula only has 12 hydrogens "H"?

a)

C4H10 (butane)

b)

C5H12 (pentane)

c)

C12H22O11 (sugar)

d)

C8H10N4O2 (caffeine)

53.
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
54.

Glycerol has a molecular molar mass of 92.09g/mol. The empirical formula is C3H8O3. What is the molecular formula for glycerol?

a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
55.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the empirical formula for this compound?

(a)  

56.
What is the best definition for subscript?
 
a)
The big number that tells you the number of molecules.
b)
The atomic number
c)
The little number that tells the number of atoms for each element.
57.
What is the best definition for coefficient?
 
a)
The big number that tells you the number of molecules.
b)
The little number that tells the number of atoms for each element.
c)
The atomic number
58.
What is the best definition for molecule? 
a)
A molecule is formed when two or more atoms join together chemically.
b)
A molecule is made of only one atom. 
59.
What is the best formula for this molecule?
a)
C5HO4
b)
C5HO7
c)
C5HO8
60.

What do you need done at the start of a stoichiometry problem?

a)

a balanced equation

b)

a certain "amount," unit, and chemical formula for your "given" &

a certain "amount" and unit for the "find?" in the problem.

c)

all the other answer choices are correct

d)

conversion factors that will help us convert from the "given" to the "find?"

e)

a Periodic Table if mass (grams) is part of the "given" or "find."

61.

What part of the balanced equation do we get the "mole ratio" from?

a)

the number of grams/mole of a substance

b)

the volume of a gas at standard temperature & pressure

c)

a ratio of the coefficient for the "find?" over the coefficient for the "given."

d)

all the other answer choices are correct

62.

If 2.02 grams of hydrogen gas (aka H2 (g) ) reacts with oxygen gas (aka O2 (g) ), which of the following would be an amount of oxygen that would include "extra" or "in excess" of what you need?

a)

32.00 grams of O2 (g)

b)

16.00 grams of O2 (g)

c)

2.00 moles of O2 (g)

d)

1.00 mol of O2 (g)

e)

22.4 Liters of O2 (g)

63.
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)
Ask for help
64.
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
65.

2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?

(a)  

66.

Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted to form AlCl3, identify the limiting reactant.

a)

AlCl3

b)

Cl2

c)

Al

67.
N2 +  3H2 −->  2NH3 
How many moles of ammonium are produced when 3 moles of nitrogen react with hydrogen?
a)
6 moles Ammonium
b)
1.5 moles ammonium
c)
9 moles ammonium
d)
9 moles hydrogen
68.
Using the balanced equation below,
 CaC₂(s)   +  2H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
69.
Using the following equation:
4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l)
How many grams of oxygen gas are needed to react with 56.8 grams of ammonia?
a)

45.1 g O2

b)

133 g O2

c)

260.77 g O2

d)

75.2 g O2

70.
When 12 moles of O2 reacts with 6 moles of C10H8, what is the limiting reactant?  
1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
71.

6Na + Fe2O3 --> 3Na2O + 2Fe


If you are provided 200g of sodium and 250 grams of iron(III) oxide, how much of excess reagent is left?

a)

232 g

b)

18 g

c)

250 g

72.

If 15 grams of copper (II) chloride react with 20 grams of sodium nitrate, how much sodium chloride can be formed? 

(a)  

73.
How many grams of ammonia (NH3) can be produced from the reaction of 28 g of nitrogen gas and 25 grams of hydrogen gas? 
a)
43 g
b)
34 moles
c)
25 grams
d)
34 grams
74.
Silver nitrate and sodium phosphate are reacted in equal amounts of 200 g each. How many grams of silver phosphate are produced? 
3AgNO3  + Na3(PO4)  --->  Ag3(PO4)  + 3NaNO3
a)

164 g

b)

200 g

c)

100 g

d)

160 moles

75.

3CaCO3 + 2FePO4 --> Ca3(PO4)2 + Fe2(CO3)3


Assuming we start with 40.5 g of CaCO3 and 45 g of FePO4, identify the limiting reactant.

a)

iron(V) phosphate

b)

calcium carbonate

c)

iron(III) phosphate

d)

calcium(II) carbonate

76.

CuCl2 + 2NaNO3 --> Cu(NO3)2 + 2NaCl

If 15.0 grams of CuCl2 react with 20.0 g of NaNO3, how much NaCl can be formed?

a)

13.0 g of NaCl

b)

98.1 g of NaCl

c)

26.3 g of NaCl

d)

17.4 of NaCl

77.

3CaCO3 + 2FePO4 --> Ca3(PO4)2 + Fe2(CO3)3

Assuming we start with 100 g of CaCO3 and 45 g of FePO4, how much of the excess reagent is left over after the reaction is complete? (yes, sig fig is off)

a)

57.3 g of sodium phosphate

b)

55.2 g of calcium carbonate

c)

25 g of calcium carbonate

d)

16.9 g of iron(III) carbonate

78.

The Law of Conservation of Matter

a)

tells how many atoms of an element are contained in one molecule or formula unit.

b)

the starting materials in a chemical reaction

c)

the new substances that are formed in a chemical reaction

d)

A law stating that atoms are not created or destroyed during a chemical reaction.

79.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

80.
Which problem is balanced?
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
81.
Balance this equation.
_SnO2 +_H2-->_Sn +_H2O
a)
1,1,2,1
b)
1,2,1,1
c)
1,2,1,2
d)
1,2,2,1
82.

___ NaClO3 ----> ___ NaCl + ___ O2

a)

1, 3, 2

b)

2,3,2

c)

2, 2,3

d)

3, 2, 2

83.
Finish a blalanced equation:
Mg(OH)2 --> __________
a)
Mg(OH)2 --> MgOH
b)
Mg(OH)2 --> MgO+ H2O
c)
Mg(OH)2 --> MgO+ H2
d)
Mg(OH)2 --> Mg+ H2O
84.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

85.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

86.
What are the products of this reaction?
Cu+ AgNO3--> 
a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
87.
Predict the products for the this reaction:
K + HCl --> 
a)
KCl + H2
b)
KHCl 
c)
KH + Cl2
d)
KCl + H
88.
Classify
FeS + HCl → H2S + FeCl2
a)
synthesis
b)
combustion
c)
single replacement
d)
double replacement
89.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)
Fe + 3 O2 → Fe2O3
b)
3 Fe + 3 O2 → 2 Fe2O3
c)
2 Fe + O2 → Fe2O3
d)
4 Fe + 3 O2 → 2 Fe2O3
90.

What is the correct way of representing hydrogen gas alone, in a reaction?

a)

2H

b)

H

c)

H2

91.

Fill in the blank. (Copper has a charge of +2)

Cu+ AgNO3--> Ag + _____

a)

Cu(NO3)2

b)

CuNO3

c)

CuAg

d)

Cu

92.

What is the oxidation number of O in a molecule? (You can click on the periodic table and make it larger)

a)

+2

b)

-1

c)

+4

d)

-2

93.

What is the oxidation number of K in a molecule? (You can click on the periodic table and make it larger)

a)

+2

b)

-1

c)

+1

d)

-2

94.

What are the products of the following synthesis reaction?

F2 + Ca →

a)

FCa

b)

F2Ca

c)

CaF2

d)

FCa

95.

What are the products of this single replacement reaction?

F2 + K3P →

a)

KF + P2

b)

F2K3 + P

c)

KF + P

96.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
97.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
98.
2Fe2O3  +  C  →  Fe  +  3CO2
You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)
a)
15.8%
b)
209.2%
c)
6435%
d)
15.5
99.
Percent yield = 100%
Theoretical yield = 88 grams
What is your actual yield?
a)
88 grams
b)
88%
c)
100 grams
d)
22%
100.
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%

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