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Worksheets

(H.Chem) 3rd Quarter Review

Total questions: 153

Worksheet time: 3hrs 33mins

Name
Class
Date
1.

How many grams are there in 3.58 moles of water?

a)

56.4 g

b)

64.5 g

c)

0.199g

d)

1.77 g

2.

How many moles of chlorine do you have from 142 g of chlorine gas (Cl2)?

a)

0.410 moles

b)

2.00 moles

c)

4.00moles

d)

0.200 moles

3.

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

a)

0.0044 g

b)

91 g

c)

110 g

d)

74 g

4.
Calculate the % composition by mass of oxygen present in H2SO4.
a)
16.3%
b)
65.25%
c)
32.6%
d)
57.14%
5.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
6.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
7.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
8.
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
9.

What is the molar mass of AgF?

a)

514.9 g/mol

b)

99.7 g/mol

c)

126.87 g/mol

d)

198.8 g/mol

10.

What is the total mass of a 0.75 mole sample of SO2?

a)

16 g

b)

24 g

c)

32 g

d)

48 g

11.

Determine the mass of 2.40 moles of C6H12

a)

201 g

b)

115 g

c)

230. g

d)

353 g

12.

What is the molar mass of calcium hydroxide, Ca(OH)2?

a)

74.1 g/mole

b)

57.1 g/mole

c)

58.1 g/mole

d)

57.1 u

13.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
14.

How many moles of magnesium are in a 20.4 g strip?

a)

0.815 mol

b)

0.820 mol

c)

0.839 mol

d)

1.84 mol

15.

Convert 5.0 mol of NH3 to grams

a)

17 g

b)

5 g

c)

85 g

d)

385 g

16.
Which conversion factor should be used to solve the following, "How many moles of argon atoms are present in 11.2 L of argon gas at STP?"
a)
1 mol = 22.4 L 
b)
1 mol = 39.95 g
c)
1 mol = 6.02x1023 atoms
d)
More than 1
17.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
18.
Which expression below show the correct method of determining the percent composition of Sodium in Na2CO3?
a)
%Na = (22.99g/106g) x 100
b)
%Na = (22.99g/106) / 100
c)
%Na = (45.98g/106g) x 100
d)
%Na = (106/45.98g) x 100
19.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
20.
Which of the following would have the highest number of moles?
a)
4g CO2
b)
15g H2O
c)
22g NaCl
d)
100g AgCl
21.
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
22.
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
23.
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
24.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg 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
25.

Cl2 + 2 KBr → Br2 + 2 KCl

How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?

a)

749 g

b)

223 g

c)

479 g

d)

814 g

26.

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

Mg + 2 H2O → Mg(OH)2 + H2

a)

62L

b)

65L

c)

31L

d)

124L

27.

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

4 NH3 + 6 NO → 5 N2 + 6 H2O

a)

5.0 L

b)

20.0 L

c)

7.5 L

d)

120.0 L

28.

2 H2 + O2 → 2 H2O

How many grams of H2O can be produced from 3.91 g of O2?

a)

1.905

b)

4.4

c)

2.2

d)

1.1

29.
Always starts with a Hydrocarbon that reacts with oxygen and produces carbon dioxide and water. 
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
30.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
31.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
32.

Hydrogen and oxygen molecules combine to form water molecules as shown in the reaction below. Given the molecules provided, which of the following is true about the products of this reaction? 

a)

2 H2O molecules are produced, O2 is the limiting reactant

b)

4 H2O molecules are produced, H2 is the limiting reactant

c)

4 H2O molecules are produced, O2 is the limiting reactant

d)

6 H2O molecules are produced, H2 is the limiting reactant

33.

P4 + 3O2 --> P4O6

How many moles of P4O6 can be made if 3 moles of P4 react with 6 moles of O2?

a)

1 mole

b)

2 moles

c)

4 moles

d)

0 moles

34.

How much water can be made if 8 moles of NH3 react with 6 moles of NO?

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

a)

5 moles

b)

6 moles

c)

12 moles

d)

18 moles

35.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
36.
CH4 + 2H2O --> CO2 + 4H2
What is the limiting reactant when 20g CH4 react with 15g H2O?
a)
CH4
b)
H2O
c)
CO2
d)
H2
37.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
38.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
39.
2 NaCl + Pb(NO3)2 --> 2 NaNO3 + PbCl2
 
How many grams of lead II chloride are produced from the reaction of 15.3 g of NaCl and 60.8 g of Pb(NO3)2? 
a)
21.5g
b)
51.1g
c)
43.4g
d)
36.4g
40.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
41.

The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield?

C6H6 + HNO3 → C6H5NO2 + H2O

a)

100%

b)

27.39%

c)

54.29%

d)

85.62%

42.

2 Fe2O3 + C → Fe + 3 CO2

You add 28.0 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)

58.8%

b)

308%

c)

6440%

d)

15.5%

43.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24
44.
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
45.

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

46.

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

47.

Given the following reaction:


B2H6 + 3 O2 → 2 HBO2 + 2 H2O


How many liters of O2 will be needed to burn 36.1 g of B2H6?

a)

87.83 liters O2

b)

12.98 liters O2

c)

67.48 liters O2

d)

0.23 liters O2

48.

Using the following equation:


2 NaOH + H2SO4 → 2 H2O + Na2SO4


How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?

a)

355 g of Na2SO4

b)

35.5 g of Na2SO4

c)

3.55 g of Na2SO4

d)

3555 g of Na2SO4

49.

Using the following equation:

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


How many moles of oxygen (O2) are needed to react with 56.8 grams of ammonia by this reaction?

a)

4.17 moles O2

b)

41.7 moles O2

c)

40.17 moles O2

d)

0.417 moles O2

50.
Question Image

Match the following equations to the correct type

a)

Synthesis

1.

2H2 + O2 --> 2H2O

b)

Decomposition

2.

NaCl --> Na + Cl

c)

Single Replacement

3.

Zn + 2 HCl --> ZnCl2 + H2

d)

Double Replacement

4.

NaBr + LiCl --> NaCl + LiBr

e)

Combustion

5.

CH4 + 2O2 --> CO2 + 2H2O

51.

Organize these options into the right categories

Categorize the following

A + B --> AB

AB --> A + B

AB + C --> AC + B

AB + CD --> AD + CB

Synthesis
Decomposition
Single Replacement
Double replacement
52.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
53.
Silver Iodide
a)
Soluble 
b)
Insoluble 
54.
KOH
a)
Soluble 
b)
Insoluble
55.
Silver acetate
a)
Soluble 
b)
Insoluble
56.
Based on the activity series, will this reaction occur?
Ni (s) + H2O (l) →
a)
Yes
b)
No
57.
Based on the activity series, will this reaction occur?
Br2 (l) + KI (aq) →
a)
Yes
b)
No
58.

Based on the activity series, will this reaction occur?
Cs (s) + HCl (aq) →

a)
Yes
b)
No
59.
A mixture contains cobalt metal, copper metal, and tin metal. This mixture is mixed with nickel nitrate. Which metals, if any, will react? 
a)
Cobalt only
b)
Copper only
c)
Tin only
d)
All 3
60.

Is this reaction balanced? If not, select the choice that best explains why it is not balanced.

Mg(NO3)2 + 2Na --> 2NaNO3 + Mg

a)

No because Mg is not balanced

b)

No because N is not balanced

c)

No because Na is not balanced

d)

No because O is not balanced

e)

yes

61.

What type of reaction is below?

CH4 + O2 --> CO2 + H2O

a)

Combination/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

62.

What would the products of this reaction be? K2O --> ?

a)

K + O

b)

K2 + O

c)

K2 + O2

d)

K + O2

e)

K2O

63.

Predict the products of this reaction: MgO + Li --> ?

a)

LiO + Mg

b)

MgO + Li

c)

Li2O + Mg

d)

LiMg + O

e)

MgLi + O

64.

Predict the products from the following reaction:

KCl + Na2SO4

a)

NaK + SO4Cl

b)

K2SO4 + NaCl

c)

KaS + ClONa

d)

KN + a

65.

Identify the species reduced in the following reaction.


Fe(s) + 2 Ag+(aq) → Fe2+(aq) + 2 Ag(s)

a)

Fe

b)

Ag

c)

none of these

d)

None of the above

66.

The below reaction is an example of _________reaction.

F2 → 2 F- + 2 e-

a)

Oxidation

b)

Reduction

c)

Neutralization

d)

decomposition

e)

combustion

67.

Find the oxidation number of Ca in CaH2

a)

-2

b)

-4

c)

+2

d)

+4

e)

0

68.

Oxidation is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

69.

Reduction is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

70.

What is the oxidation state of Nitrogen in N2 (g)?

a)

4

b)

6

c)

2

d)

0

71.

In a redox reaction, the species reduced

a)

gains electrons and is the oxidizing agent

b)

loses electrons and is the oxidizing agent

c)

loses electrons and is the reducing agent

d)

gains electrons and is the reducing agent

72.

What is the oxidation number of Nitrogen in HNO3

a)

-7

b)

-5

c)

+5

d)

+7

e)

+2

73.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
74.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
75.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
76.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
77.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
78.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
79.

When the equation is balanced what are the correct coefficients?



a)

1, 1, 2

b)

 1, 3, 1

c)

2, 2, 3

d)

2, 3, 2

80.

What are the correct coefficients when the equation is balanced?

a)

2, 3, 4

b)

4, 3, 2

c)

1, 1, 2

d)

2, 1, 1

81.

Which of the following is an example of a synthesis reaction?

a)
b)
c)
d)
82.

Which of the following is an example of a redox decomposition reaction?

a)

b)

c)

d)

83.

Which of the following is an example of a single replacement reaction?

a)

b)

c)

d)

84.

Which of the following is an example of a double replacement reaction that forms a precipitate?

a)

b)

c)

d)

85.

When balanced, the correct coefficients for the equation are:

a)

1, 3, 3, 1

b)

1, 3, 2, 1

c)

2, 3, 3, 1

d)

1, 1, 3, 1

86.

When balanced, the correct coefficients for the equation are:

a)

2, 1, 3, 1

b)

1, 2, 1, 2

c)

1, 2, 2, 1

d)

2, 1, 1, 2

87.

When balanced, the correct coefficients for the equation are:

a)

3, 1, 2, 1

b)

1, 2, 3, 4

c)

2, 1, 2, 1

d)

1, 2, 1, 1

88.

When balanced, the correct coefficients for the reaction are:

a)

1, 1, 1, 1

b)

1, 2, 1, 1

c)

2, 1, 1, 2

d)

2, 1, 2, 1

89.

When balanced, the correct coefficients are:

a)

2, 2, 2

b)

2, 2, 3

c)

3, 2, 2

d)

1, 2, 3

90.

Why must the number of atoms on either side of the arrow be equal to each other in a chemical equation?

a)

to abide by the law of conservation of energy

b)

to abide by law of conservation of mass

c)

to abide by the law of fundamental equations

d)

because everything must be even for the universe to stay in balance

91.

What type of reaction involves a fuel being burned in the presence of oxygen in order to produce carbon dioxide and water?

a)

single replacement

b)

synthesis

c)

double replacement

d)

combustion

92.

Identify the type of the following reaction.


__CH4 + __ O2 → __ CO2 + __ H2O

a)

Single Replacement

b)

Combustion

c)

Synthesis

d)

Double Replacement

e)

Neutralization

93.
What element is being Oxidized?
a)
N
b)
H
c)
O
d)
S
94.
What element is being Reduced?
a)
N
b)
H
c)
O
d)
S
95.
What are the coefficients when the equation is balanced?
a)
2 + 3 --> 2 + 3 + 4
b)
1 + 3 --> 1 + 3 + 2
c)
2 + 4 --> 2 + 3 + 2
d)
1 + 1 --> 1 + 1 + 1
96.

What is oxidation number of Cr in Cr2O7 2- ?

a)
-2
b)
+2
c)
+6
d)
+12
97.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
98.
If in a reaction, copper is reduced; its number of electrons has:
a)
Increased
b)
Decreased
c)
Remained Constant
d)
Varies Randomly
99.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
100.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
101.

Mg + PbCl2 --> MgCl2 + Pb. Which statement correctly describes the oxidation and reduction that occur?

a)

Mg is oxidized and Cl- is reduced

b)

Mg is oxidized and Pb+2 is reduced

c)

Mg is reduced and Cl- is oxidized

d)

Mg is reduced and Pb+2 is oxidized

102.

Predict the products that will form if aluminum oxide react with potassium metal?

a)

potassium aluminum oxide

b)

aluminum + potassium oxide

c)

potassium aluminum + oxygen gas

d)

oxygen gas + potassium metal + aluminum metal

103.

What are the coefficients for the following reaction?

​ ___C2H6 + ___O2 ----> ___CO2 + ____H2O

a)

1,2,2,3

b)

2,5,4,3

c)

2,7,4,6

d)

1,3,2,3

104.

A reaction in which a compound breaks down into two or more substances is a(n):

a)

single replacement

b)

double replacement

c)

combustion

d)

synthesis

e)

decomposition

105.

Use the activity series to determine if the following reaction will occur:

__Fe + ___Al2O3 ----> ___Al + ____Fe2O3

a)

Yes

b)

No

c)

Not enough information to determine

106.

Use the activity series to determine if the following reaction will occur:

4 Al + 3 PbO2 ----> 3 Pb + 2 Al2O3

a)

Yes

b)

No

c)

Not enough information to determine

107.

Predict the products: C2H6 + O2 --> ?

a)

H2O + O2

b)

CO2 + H2O

c)

C + O2

d)

CO2 + H2O2

e)

CH + O2

108.

Predict the products from this reaction: ZnCl2 + Mg --> ?

a)

MgCl2 + Zn2

b)

Zn2Mg + Cl2

c)

MgCl2 + Zn

d)

ZnCl + Mg

e)

MgCl + Zn

109.

What element is required for a combustion reaction?

a)

nitrogen

b)

hydrogen

c)

silicon

d)

oxygen

e)

carbon

110.

What is the precipitate that will form from the following reaction:

Pb(NO3)2 (aq) + KI (aq) --> PbI2 (?) + KNO3 (?)

a)

PbI2

b)

KNO3

111.

What is the precipitate that will form from the following reaction:

Pb(NO3)2 (aq) + NaOH (aq) -->

a)

Pb(OH)2

b)

NaNO3

c)

PbNa

d)

NO3OH

112.

Pb(NO3)2 (aq) + KI (aq) -->

What substance forms the precipitate in this reaction?

a)

Lead Nitrate

b)

Potassium Iodide

c)

Lead Iodide

d)

Potassium Nitrate

113.

Predict if a precipitate will form from the following reaction:

KI (aq) + NaOH (aq) --> KOH (?) + NaI (?)

a)

precipitate

b)

no reaction

114.

Pb(NO3)2 (aq) + NaI (aq) --> PbI2 (?) + NaNO3 (?)

What substance forms the precipitate in this reaction?

a)

Lead Nitrate

b)

Sodium Iodide

c)

Lead Iodide

d)

Sodium Nitrate

115.

Based on the activity series, which metal could X represent in the reaction below?

X + Calcium nitrate —> Calcium + X nitrate

a)

Ba

b)

Fe

c)

Mg

d)

Zn

116.
Will silver react with magnesium chloride solution?
a)
yes
b)
no
117.

What type of reaction is best used to describe the following.. (don't worry about balancing):

CaO(s) + H2O(l) → Ca(OH)2 (s)

a)

Redox Decomposition

b)

Redox Synthesis

c)

Simple Synthesis

d)

Simple Decomposition

118.

Predict the product(s) of this reaction (don't worry about balancing):

Mg + HCl →

a)

MgHCl

b)

MgCl2 + H2

c)

MgCl2 + H

d)

MgCl + H2

119.

Based on the activity series, which metal could X represent in the reaction below?

X + Ca (NO3)2 --> Ca + X (NO3)2

a)

Ba

b)

Fe

c)

Mg

d)

Zn

120.

Which is the correct net ionic equation for the reaction of AgNO3 + CaCl2 -->?

a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
121.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
122.
What is the oxidation number of N in NO2-1?
a)
-3
b)
+4
c)
-2
d)
+3
123.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
124.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
125.
H3PO4 is an example of a ...
a)
acid
b)
base
c)
salt
126.

Complete the following reaction:

HCl + Mg(OH)2 →

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

127.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

128.

In this equation,

CuCl2+ NaOH → Cu(OH)2 + NaCl

Which product is insoluble?

a)

copper(II) hydroxide

b)

sodium chloride

c)

sodium hydroxide

d)

copper(I) hydroxide

129.

MgClO3(s) ----> MgCl2(s) + O2(g)

a)

Simple Synthesis

b)

Simple Decomposition

c)

Redox Synthesis

d)

Redox Decomposition

130.

MgCl2(s) + O2(g) ----> MgClO3(s)

a)

Redox Synthesis

b)

Simple Decomposition

c)

Simple Synthesis

d)

Redox Decomposition

131.

What is the best way to categorize the following reaction?

CaCO3(s) ----> CaO(s) + CO2(g)

a)

Simple Synthesis (or combination)

b)

Simple Decomposition

c)

Redox Decomposition

d)

Redox Synthesis

132.

Is the following equation balanced?

4Fe + 3O2 ---> 2Fe2O3

a)

YES

b)

NO

133.

Net Ionic equations include all ions. even the spectator ions.

a)

True

b)

False

134.

Spectator ions ALWAYS participate in the reaction.

a)

True

b)

False

135.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
136.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
137.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
138.

In a redox reaction, spectator ions...

a)

become oxidised

b)

become reduced

c)

remain unchanged

139.

What is the oxidation number of iodine in KIO3?

a)

0

b)

-1

c)

+5

d)

+1

140.

What is the oxidation number of nitrogen in N2?

a)

-3

b)

0

c)

+4

d)

-1

141.

What is the spectator ion in the following reaction?

3 Ca(S) + 2 AlCl3 (aq)--> 3 CaCl2(s) +  2 Al(s)

a)

Ca2+

b)

Al3+

c)

Cl-

d)

CaCl2

142.
Which one is an empirical formula?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
143.
What is the empirical formula for C3H8
a)
CH
b)
C3H8
c)
C6H16
d)
CH2.7
144.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
145.
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
146.

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

147.

What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?

a)

NO

b)

N2O4

c)

N2O3

d)

N2O5

148.

A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

149.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)

C3H8

b)

CH4

c)

C2H2

d)

C4H10

150.

Given the following, determine the empirical formula: 42.07% sodium, 18.89% phosphorus, and 39.04% oxygen.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

Na3PO3

151.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
152.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
153.
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

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