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Worksheets

3rd Nine Weeks review

Total questions: 92

Worksheet time: 3hrs 56mins

Name
Class
Date
1.

In the diagram, letter D represents a

a)

subscript

b)

coefficient

c)

product

d)

equation

2.

In the diagram, letter E represents a

a)

subscript

b)

coefficient

c)

product

d)

equation

3.
Which are the reactants in the equation shown?
a)
H2O and CO2
b)
O2 and CH4
4.

Which is the product in the reaction shown?

a)

Al2O3

b)

Al

c)

O2

5.
What describes the reactant atoms in the equation shown?
a)
Al= 4, O= 3
b)
Al= 1, O= 1
c)
Al= 4, O= 6
d)
Al= 6, O= 1
6.

How does the mass of products compare to the mass of reactants in a chemical reaction?

a)

reactants = products

b)

reactants > products

c)

reactants < products

7.

In the reaction shown below, 12 grams of AB break down into 8 grams of product A and an unknown amount of product B.


Using the law of conservation of mass, what will the mass of product B be?

a)

4 grams

b)

8 grams

c)

12 grams

d)

20 grams

8.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

9.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

10.

What reaction has the following general formula:

A + B --> AB

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

11.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

12.

What type of reaction is the following:
BaCl2+2KI −> 2KCl + BaI2BaCl_2+2KI\ ->\ 2KCl\ +\ BaI_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

13.

What type of reaction is the following:
2KI −> 2K + I22KI\ ->\ 2K\ +\ I_2  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

14.

What type of reaction is the following:
C11H24+17O2−> 11CO2 + 12H2OC_{11}H_{24}+17O_2->\ 11CO_2\ +\ 12H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

15.

What type of reaction is the following:
2NaHCO3−> Na2CO3+CO2+H2O2NaHCO_3->\ Na_2CO_3+CO_2+H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

16.

What type of reaction is the following:
Zn + 2HCl −> ZnCl2+H2Zn\ +\ 2HCl\ ->\ ZnCl_2+H_2

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

17.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

18.

Which of the following is an element?

a)

potassium chloride (KCl)

b)

water (H2O)

c)

carbon (C)

d)

calcium carbonate (CaCO3)

19.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

20.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
21.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
22.
__H2O2 --> __H2O + __O2
a)
already balanced
b)
2,1,1
c)
2,2,1
d)
2,1,2
23.
__NaClO3 --> __NaCl + __O2
a)
2,2,2
b)
2,2,3
c)
3,2,2
d)
1,2,3
24.
__C6H12O6 + __O2 --> __H2O + __CO2
a)
1,6,6,6
b)
already balanced
c)
1,6,1,6
d)
2,12,12,12
25.
_AgNO3 + _Cu →_Cu(NO3)2 + _Ag
a)
2 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 1 Ag
b)
2 AgNO3 + 1 Cu → 1 Cu(NO3)2 + 2 Ag
c)
1 AgNO3 + 2 Cu → 2 Cu(NO3)2 + 1 Ag
d)
3 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 2 Ag
26.
Balance this equation:
MgCl2 --> Mg4+ Cl2
a)
It's already balanced.
b)
4MgCl2 --> Mg4+ 4Cl2
c)
4MgCl2 --> Mg4+ 5Cl2
27.
Balance this equation:
 2Li + Cl2 -> LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
28.
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. 
29.
__(NH4)3PO4 + __Pb(NO3)4 --> __Pb3(PO4)4 + __NH4NO3
a)
2,1,1,6
b)
1,2,2,3
c)
4,3,1,12
d)
4,2,1,12
30.

Is the following reaction balanced?

Ca+CuF2→CaF2+CuCa+CuF_2\rightarrow CaF_2+Cu  

a)

Yes

b)

No

31.

For the following chemical reaction, which substance is a reactant?

2HBr + Mg(OH)2 → MgBr2 +2H2O2HBr\ +\ Mg\left(OH\right)_2\ →\ MgBr_2\ +2H_2O  

a)

MgBr2MgBr_2  

b)

BrBr  

c)

Mg

d)

HBr

32.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

33.

One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

34.

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

35.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

36.

A mole is:

a)

The SI unit for mass

b)

The SI unit for the amount of a substance

c)

The SI unit for volume

d)

The SI unit for area

37.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
38.

What converting from moles to the number of particles, moles is multiplied by:

a)

an equivalent value

b)

a conversion factor

c)

the number of atoms in the formula

d)

the mass of the substance

39.

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

40.

What is correct equation that should be used to determine how many molecules there are in 0.75 moles of (NH4)3PO4?

a)
b)
c)
d)
41.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

42.

How many moles of Na contain 1.45 x 1021 atoms of Na?

a)

8.73 x 1044 moles

b)

8.73 moles

c)

0.00241 moles

d)

2.41 x 1044 moles

43.
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 
44.

What is the molar mass of Oxygen?

a)

8 grams

b)

8 moles

c)

16 grams

d)

16 moles

45.
Molar mass is in units of ________.
a)

grams

b)

grams/mole

c)

mole

d)

moles/gram

46.

Calculate the Molar Mass of MgO?

a)

40.3 grams

b)

24.3 grams

c)

16 grams

d)

39 grams

47.

What is the molar mass of PbSO4?

a)

303.3 g/mol

b)

255.3 g/mol

c)

163.9 g/mol

d)

372.3 g/mol

48.

Determine the mass of 4.20 moles of C6H12

a)

352.8 grams

b)

0.0499 grams

c)

337 grams

d)

2.53 x 1024 grams

49.

How many moles are in 78 grams of Li3N?

a)

34.83 moles

b)

2.23 moles

c)

78 moles

d)

20.82 moles

50.

How many moles are in 19.5 grams of Sodium?

a)

19.5 moles

b)

0.85 moles

c)

22.99 moles

d)

8.5 moles

51.

When a question gives you moles and asks you to calculate volume, where do you find the volume to use?

a)

22.4 L

b)

22.4 L/mole

c)

Periodic Table

L/mole

d)

6.02 x 1023 L/mole

52.

When converting mass to moles, what conversion factor is needed?

a)

mass = 1 mole

b)

mass = 1 gram

c)

mass = 1 Liter

d)

mass = 1 atom

53.

When converting volume to moles, what conversion factor is needed?

a)

22.4 grams = 1 mole

b)

22.4 L = 1 mole

c)

22.4 moles = 1 Liter

d)

6.02 L = 1 mole

54.

In Chemistry, STP stands for ___?

a)

Scientifically Treated Petroleum

b)

Standard Temperature and Pressure

c)

Stone Temple Pilots

d)

Segmentation, Targeting, & Positioning

55.
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
56.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

57.
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
58.
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
59.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
60.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
61.
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
62.
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
63.
 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
64.
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)
45.08 g O2
b)
133.33 g O2
c)
260.77 g O2
d)
75.92 g O2
65.

3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe

Identify the mole ratios for the following pairs:

​ ​ ​ (a)   Mg : ​ (b)   Fe

​ (c)   Fe2O3 : ​ (d)   Fe

​ 1 Fe2O3 : ​ (e)   MgO

Choose from the below words
3
2
1
66.

1 CH4 + 2 O2 → 1 CO2 + 2 H2O

How many moles of carbon dioxide (CO2) are produced from the combustion of 110.0 g of CH4 (molar mass = 16 g)?

a)

13.7 mol

b)

2.75 mol

c)

6.85 mol

d)

6.11 mol

67.

Balance the following reaction:

​ (a)   CaC2 + ​ (b)   H2O → ​ (c)   C2H2 + ​ (d)   Ca(OH)2

Choose from the below words
1
2
68.
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
69.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
70.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
71.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
72.
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
73.
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
74.
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
75.
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
76.
If 15 grams of copper (II) chloride react with 20 grams of sodium nitrate, how much sodium chloride can be formed? 
a)
13.04 g
b)
130.4 moles
c)
130.4 g
d)
13.04 moles
77.
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
78.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
79.
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
80.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
81.
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
82.
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
83.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
84.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
a.  Mg +  2HCl --> MgCl2  +  H2   
b.  a.  Mg +  2HCl --> MgCl2  +  H2   

a)
Mg
b)
H2
c)
MgCl2
d)
HCl
85.

What is the result when 2.40 g of Mg reacts with 10.0 g of O2?

a)

Both react completely

b)

No reaction occurs

c)

Mg is the limiting reagent

d)

O2 is the limiting reagent

86.

1 P4 + 3 O2 → 2 P2O3

Match the ratio to the correct substances:

a)

1:3

1.

P:O2

b)

1:2

2.

P:P2O3

c)

3:2

3.

O2:P2O3

d)

3:1

4.

O2:P

e)

2:3

5.

P2O3:O2

87.

Where can you find the data you need to calculate the molar mass of a compound?

a)

Sheet of formulas and constants

b)

The reaction equation

c)

The periodic table

d)

It must be given in the question

88.

What do Coefficients (like the 3 in front of Hydrogen) in a reaction equation indicate?

a)

The number of atoms in the molecule.

b)

How much to multiply the molar mass by for this reaction.

c)

How many of that molecule are needed for one run of the reaction.

d)

How many moles of that molecule are present in the reaction.

89.

If 5.0 grams of A react with 3.0 grams of B to produce C, and after the reaction, there are still 1.0 grams of B left, which is the limiting reagent?

a)

A

b)

B

c)

C

d)

Both A and B

90.

Why is the actual yield of a reaction typically less than the theoretical yield?

a)

Incomplete reactions.

b)

Measurement errors.

c)

Formation of by-products.

d)

All of the these.

91.

What do Coefficients (like the 3 in front of Hydrogen) in a reaction equation indicate?

a)

The number of atoms in the molecule.

b)

How much to multiply the molar mass by for this reaction.

c)

How many of that molecule are needed for one run of the reaction.

d)

How many moles of that molecule are present in the reaction.

92.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich

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