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Stoichiometry, Limiting Reactant, & Percent Yield Quiz

Total questions: 167

Worksheet time: 10hrs 58mins

Name
Class
Date
1.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
2.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
3.

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%

4.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
5.
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%
6.
Lead nitrate can be decomposed by heating.  What is the % yield of the decomposition reaction if 7.4g Pb(NO3)2 are heated to give 4.1 g PbO?
2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)
a)
82%
b)
44%
c)
56%
d)
67%
7.

What is the formula for percent yield?

a)

actual yieldtheoretical yield×100\frac{actual\ yield}{theoretical\ yield}\times100

b)

theoretical yieldactual yield×100\frac{theoretical\ yield}{actual\ yield}\times100

c)

moles Amoles B\frac{moles\ A}{moles\ B}

d)

grams Agrams B\frac{grams\ A}{grams\ B}

8.

If you are converting from grams of substance A to grams of substance B, drag the correct order of the conversion process:

​ (a)   ---> ​ (b)   ---> ​ (c)   ---> ​ (d)  

Choose from the below words
Grams A
Moles A
Moles B
Grams B
9.

Based on the following equation and question, choose the actual yield:

 Zn  +  2HCl   →   ZnCl2  +  H2Zn\ \ +\ \ 2HCl\ \ \ \rightarrow\ \ \ ZnCl_2\ \ +\ \ H_2

20 g of  ZnCl2ZnCl_2(136.286 g/mol) is formed in a lab. What is percent yield if 10 g of HCl (36.453 g/mol) is consumed?

a)

44.5%

b)

35.4%

c)

10.6 %

d)

26.8 %

10.

Calculate percent yield based on the following information:

Actual Yield: 50

Theoretical Yield: 60

a)

0.8333 %

b)

83.33 %

c)

120 %

d)

1.2 %

11.

Which of the following reactions has the lowest percent yield?

a)

Theoretical yield 25.7 g; actual yield 23.2 g

b)

Theoretical yield 42.1 g; actual yield 39.9 g

c)

Theoretical yield 18.2 g; actual yield 15.6 g

d)

Theoretical yield 93.4 g; actual yield 87.9 g

12.

List one reason why the actual yield is lower than the theoretical yield.

(a)  

13.
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
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.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
16.
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
17.
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
18.
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
19.
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
20.
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
21.

How many grams are in 7.8 moles of NaCl?

a)

476 grams

b)

460 grams

c)

452 grams

d)

462 grams

22.
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
23.
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
24.
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
25.
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
26.
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%
27.
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
28.
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
29.
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
30.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
31.

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

32.
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
33.

It refers to the substance(s) that are considered to be "ingredients" of a chemical reaction.

a)

reactants

b)

products

c)

catalysts

d)

enhancers

34.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
35.

1 Cheese + 2 Bread --> 1 grilled cheese

How many grilled cheeses can you make with 26 slices of bread and 14 pieces of cheese?

a)

14

b)

13

c)

26

36.
The excess reactant
a)
.
b)
is used up first
c)
is the reactant that is left over
d)
.
37.

The Formula to make S'mores is:

2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), how many S'mores can you make?

a)

5

b)

4

c)

8

d)

42

38.
A reactant that remains after a chemical reaction stops
a)
stoichiometry
b)
mole ratio
c)
excess reactant
d)
limiting reactant
39.

Why is it important to identify the limiting reagent?

a)

The limiting reagent speeds up the reaction.

b)

The limiting reagent controls the amount of product formed.

c)

If there is no limiting reagent, the reaction will not occur.

d)

No stoichiometry calculations can be done without a limiting reagent.

40.

Using the diagram, determine the limiting reactant, the product formed is water.

a)

oxygen

b)

hydrogen

c)

none of the reactant are limiting

d)

both hydrogen and oxygen

41.
2. True or False?
A chemical reaction stops before the limiting reagent is used up.
a)
True
b)
False
42.
1 Body + 4 Tires --> 1 car
How many cars can you make with 92 tires and 34 bodies? 
a)
23
b)
34
c)
68
d)
46
43.
1 Body + 4 Tires --> 1 car
How many cars can you make with 92 tires and 34 bodies? 
In this senario the tires would be the _____________  reactant. 
a)
Limiting 
b)
Excess 
44.

The Formula to make S'mores is:

2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), what is the limiting reactant?

a)

Chocolate pieces (C)

b)

Marshmallows (M)

c)

Graham Cracker Halves (G)

d)

There is not a limiting reactant present

45.

Match the following

a)

Synthesis

1.

Multiple reactants form a single compound.

b)

Decomposition

2.

A single compound breaks down into simpler substances

c)

Single Displacement

3.

One element replaces another element in a compound

d)

Double Displacement

4.

Ions in two compounds exchange places to form two new compounds

e)

Combustion

5.

Elemental oxygen is a reactant.

46.

What must be done FIRST to solve a stoichiometry problem?

a)

Write and balance a chemical equation.

b)

Mathematically determine the limiting reactant.

c)

Mathematically determine the excess reactant.

d)

Ensure all quantities are in grams.

47.

The mole ratio number of a substance is represented by its

a)

chemical formula

b)

subscripts

c)

superscripts

d)

coefficient

48.

What type of chemical reaction is this one?

Al(OH)3 --> Al2O3 + H2O

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Displacement

49.

What type of chemical reaction is this one?

Ca + MgCl2 --> CaCl2 + Mg

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Displacement

50.

What type of chemical reaction is this one?

CuO + CO2 --> CuCO3

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Displacement

51.

3KOH + H3PO4 --> K3PO4 + 3H2O

a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Double displacement

52.
What kind of reaction is this:
4Fe  +  3O2 →   2Fe2O3 
a)

Synthesis

b)

Decomposition

c)

Single Displacement 

d)

Double Displacement

53.
What kind of reaction is this:
2H2O2 →2 H2O + O2
a)

Synthesis

b)

Decomposition

c)

Single Displacement 

d)

Combustion

54.

Classify the following chemical reaction


BaCl2(aq) + K2CrO4(aq) --> BaCrO4(s) + 2KCl(aq)




a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

55.

Classify the follow chemical reaction.


2C6H6(l) + 15O2 --> 6H2O(l) + 12CO2(g)

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

56.

Identify the type of chemical reaction pictured above

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

57.

Identify the type of chemical reaction picture above

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

58.
3 HBr + 1 Al(OH)3 ----> 3 H­2O + 1 AlBr3
a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Double displacement

59.
Pb + FeSO4 ----> PbSO4 + Fe
a)

Synthesis

b)

Decomposition

c)

Single displacement

d)

Double displacement

60.

What reaction has the following general formula:

A + CD --> C + AD

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

61.

What is the left part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical equation

62.

What is the right part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical Equation

63.

What is the little number after an element in a chemical equation called?

Example: H2

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

64.

Is the following equation balanced?

Al + O2 ---> 2Al2O3

a)

YES

b)

NO

65.

What is the number before a chemical formula called?

Example: 2H2 + O2 ---> 2H2O

a)

Coefficient

b)

Atom

c)

Subscript

d)

Equation

66.

What is the Law of Conservation of Mass?

a)

It states that matter cannot be created or destroyed.

b)

It states that energy cannot be created or destroyed.

c)

It states that matter can be created or destroyed.

d)

It states that sound can be created or destroyed.

67.

What are the numbers that you CANNOT change in a chemical equation? 

a)
Coefficient
b)
Products
c)
Reactants
d)

Subscripts

68.

What is the right ratio of chemicals for the balanced chemical equation?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 2,4
d)
1,2 --> 2,1
69.

What is the right ratio of chemicals for the balanced chemical equation?

__CO + __Fe2O3--> __Fe + __CO2

a)
3,1 --> 2,3
b)
3,2 --> 1,1
c)
3,2 --> 2,4
d)
3,2 --> 2,1
70.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
71.
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
72.
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
73.
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
74.
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
75.
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
76.
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
77.

What is the balanced chemical equation for the reaction between hydrochloric acid and calcium carbonate when the products of the reaction are calcium chloride, carbon dioxide, and water?

a)

HCl + CaCl2 → CaCO3 + CO2 + H2O

b)

HCl + CaCO3 → CaCl2 + CO2 + H2O

c)

2HCl + CaCO3 → CaCl2 + CO2 + H2O

d)

2HCl + CaCl2 → CaCO3 + CO2 + 2H2O

78.

The reaction of 5.0 grams of fluorine with excess chlorine produced 5.6 grams of ClF3. What percent yield of ClF3 was obtained?

Cl2 + 3F2 → 2ClF3

a)

58%

b)

69%

c)

76%

d)

86%

79.

What is the limiting reactant in the reaction shown?

a)

ammonia

b)

nitrogen

c)

hydrogen

d)

There is no limiting reactant.

80.

Which of the following is NOT part of a conversion factor we studied that equals 1 mole?

a)

grams from the periodic table

b)

22.4 Liters

c)

22.4 meters

d)

6.02 x 10^23 particles (atoms, molecules)

81.

Two or more chemical species combine to form a more complex product.

a)

Decomposition Reaction

b)

Synthesis Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

82.

Compares the hands-on results to the calculated predictions.

a)

Theoretical yield

b)

Actual yield

c)

Percent yield

d)

Probable yield

83.

The amount that according to the DA (calculated) you should get if everything is just perfect.

a)

Theoretical yield

b)

Actual yield

c)

Percent yield

d)

Probable yield

84.

A reactant that is totally consumed when the chemical reaction is completed.

a)

Theoretical Reactant

b)

Excess Reactant

c)

Limiting Reactant

d)

Actual Reactant

85.

What type of reaction is 2NaCl --> 2Na + Cl2?

a)

Decomposition Reaction

b)

Synthesis Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

86.

How do you know an equation is balanced?

a)

The coefficients on the left equal the coefficients on the right.

b)

The subscripts on the left equal the subscripts on the right.

c)

There are an equal number of each type of atom on both sides of the arrow

d)

The elements on the left are the same as the elements on the right.

87.

The amount (usually mass) that you measured when you did the experiment.

a)

Theoretical yield

b)

Actual yield

c)

Percent yield

d)

Probable yield

88.

What is the first step in solving a stoichiometry problem?

a)

Note the unit of the given substance.

b)

Put the number and unit of the given at the beginning.

c)

Convert the unit of the given to moles if it does not start with moles.

d)

Writing the balanced chemical equation for the reaction.

89.

Atoms or compounds that are generated as a result of a chemical reaction (RIGHT SIDE)

a)

Products

b)

Reactants

c)

Excess Reactant

d)

Limiting Reactant

90.

In stoichiometry, what step always come after your unit is in moles?

a)

molar mass

b)

mole to mole ratio

c)

percent yield

d)

coefficients

91.

Which of the following shows the steps to go from the grams of the given to the grams of the unknown?

a)

molar mass (given) to molar ratio to molar volume (unknown)

b)

molar mass (given) to molar ratio to molar mass (unknown)

c)

molar ratio to molar mass (unknown)

d)

molar mass (given) to molar ratio to

Avogadro's to molar mass (unknown)

92.

The study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction.

a)

Percent yield

b)

Stoichiometry

c)

Types of Reactions

d)

Balancing

93.

The ____ in a balanced chemical reactions gives the MOLE RATIO used in stoichiometry problems.

a)

coefficients

b)

reactants

c)

subscripts

d)

products

94.

One reactant is exchanged for one ion of a second reactant.

a)

Decomposition Reaction

b)

Synthesis Reaction

c)

Single Replacement Reaction

d)

Double Replacement Reaction

95.

When you need to convert from moles of the given to the moles of the unknown, where do you find the information for the conversion factor?

a)

The map

b)

The balanced equation

c)

The question itself

d)

The periodic table

96.

How do you convert the given from liters to grams of an unknown substance?

a)

molar mass (given) to molar ratio to molar volume (unknown)

b)

molar volume (given) to molar ratio to molar mass (unknown)

c)

molar mass (given) to molar ratio to Avogadro's to molar mass (unknown)

d)

molar ratio to molar mass (unknown)

97.

What shows how many atoms or ions are within a compound?

a)

Coefficients

b)

Reactants

c)

Subscripts

d)

Products

98.

If the given for a mole problem is 2.45 g, how many significant figures can the final answer have?

a)

1

b)

2

c)

3

d)

As many as the calculator will show.

99.

What is the percent yield if the actual yield is 20g and the theoretical yield is 25g?

a)

125%

b)

5%

c)

80%

d)

50%

100.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
101.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
102.

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%

103.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
104.
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%
105.
Lead nitrate can be decomposed by heating.  What is the % yield of the decomposition reaction if 7.4g Pb(NO3)2 are heated to give 4.1 g PbO?
2Pb(NO3)2 (s)→2PbO(s)+4NO2(g)+O2(g)
a)
82%
b)
44%
c)
56%
d)
67%
106.

What is the formula for percent yield?

a)

actual yieldtheoretical yield×100\frac{actual\ yield}{theoretical\ yield}\times100

b)

theoretical yieldactual yield×100\frac{theoretical\ yield}{actual\ yield}\times100

c)

moles Amoles B\frac{moles\ A}{moles\ B}

d)

grams Agrams B\frac{grams\ A}{grams\ B}

107.

If you are converting from grams of substance A to grams of substance B, drag the correct order of the conversion process:

​ (a)   ---> ​ (b)   ---> ​ (c)   ---> ​ (d)  

Choose from the below words
Grams A
Moles A
Moles B
Grams B
108.

Based on the following equation and question, choose the actual yield:

 Zn  +  2HCl   →   ZnCl2  +  H2Zn\ \ +\ \ 2HCl\ \ \ \rightarrow\ \ \ ZnCl_2\ \ +\ \ H_2

20 g of  ZnCl2ZnCl_2(136.286 g/mol) is formed in a lab. What is percent yield if 10 g of HCl (36.453 g/mol) is consumed?

a)

44.5%

b)

35.4%

c)

10.6 %

d)

26.8 %

109.

Calculate percent yield based on the following information:

Actual Yield: 50

Theoretical Yield: 60

a)

0.8333 %

b)

83.33 %

c)

120 %

d)

1.2 %

110.
Which of the following do you get through measuring its mass? (No calculations)
a)
percent yield
b)
theoretical yield
c)
actual yield
d)
limiting reagent
111.

Which of the following reactions has the lowest percent yield?

a)

Theoretical yield 25.7 g; actual yield 23.2 g

b)

Theoretical yield 42.1 g; actual yield 39.9 g

c)

Theoretical yield 18.2 g; actual yield 15.6 g

d)

Theoretical yield 93.4 g; actual yield 87.9 g

112.

List one reason why the actual yield is lower than the theoretical yield.

(a)  

113.

List one reason why the theoretical yield is less than the actual yield

(a)  

114.

1 Cl2 + 2 KBr → 1 Br2 + 2 KCl

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

​ (a)   + 35 = 74g x 2 = 148g 39 + ​80 = ​ (b)   g x 2 = 238g

​ (c)   / ​ (d)   x 148 = ​ (e)   g

Choose from the below words
39
119
356
238
221
115.

1 B2H5 + 3 O2 → 2 HBO2 + 2 H2O

What mass of O2 will be needed to burn 36.1 g of B2H5?

16 x 2 = ​ (a)   x 3 = 96 g (11 x 2) + (1 x 5) = 27 g

​ (b)   / ​ (c)   x ​ (d)   = ​ (e)   g

Choose from the below words
32
36.1
27
96
128.356
116.

2 Al + 3 H2SO4 → 1 Al2(SO4)3 + 3 H2

How many grams of aluminum sulfate (Al2(SO4)3) would be formed if 250.0 g sulfuric acid (H2SO4) completely reacted with aluminum?

(27x2) + (​ (a)   x3) + (16x12) = 342 g (1x6) + (32x3) + (16x12) = 294 g

​ (b)   ÷ ​ (c)   x ​ (d)   = ​ (e)   g

Choose from the below words
32
250.0
294
342
290.81
117.
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
118.
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
119.

How many molecules are in 9.4 moles of ibuprofen?

a)
5.66
b)
5.66x1024
c)
0.705
d)
1.25x1023
120.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
121.
Question Image

Match the following...

a)

You convert moles to grams by...

1.

multiplying by the molar mass

b)

You convert liters to moles by...

2.

dividing by 22.4L

c)

You convert moles to particles by...

3.

multiplying my avagadro's constant

d)

You convert grams to moles by...

4.

dividing by the molar mass

e)

You convert moles to liters by...

5.

multiplying by 22.4L

122.

True/False: Before you begin, you must be sure your equation is balanced

a)

True

b)

False

123.

Converting from gram A to gram B, the first step is to

a)

Convert from mole A to mole B

b)

Convert from mole B to gram B

c)

Convert from gram A to mole A

124.

When you multiply for each step you are using a fraction, called a

a)

conversion factor

b)

percentage

c)

multiplier

d)

prefix

125.

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

a)

29%

b)

43%

c)

57%

d)

73%

126.

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

a)

29%

b)

43%

c)

57%

d)

73%

127.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

128.

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%

129.

What percentage of the total atomic mass of lithium phosphide (Li3P) is composed of lithium? Hint - consider all three atoms of lithium in your calculation.

a)

13%

b)

29%

c)

40%

d)

60%

130.

What percentage of the total atomic mass of lithium phosphide (Li3P) is composed of phosphorus?

a)

13%

b)

29%

c)

40%

d)

60%

131.

What percentage of the total atomic mass of calcium nitrate (Ca(NO3)2) is composed of nitrogen? Hint - another way to think of calcium nitrate is Ca(NO3)(NO3).

a)

17%

b)

24%

c)

29%

d)

59%

132.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
133.
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
134.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
135.
What is the percentage of oxygen in carbon dioxide? (CO2)
a)
27.3%
b)
72.7%
c)
30%
d)
70%
136.
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
137.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
138.
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
139.
What is the percentage of chlorine in sodium chloride? (NaCl)
a)
60.7%
b)
39.3%
c)
60%
d)
40%
140.
What is the percentage of iron in iron(III)oxide?
a)
30%
b)
70%
c)
40%
d)
60%
141.
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
142.
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
143.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
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.

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

146.

Calculate the percent water in strontium chloride hexahydrate

a)

6.76%

b)

59.45%

c)

68.21%

d)

40.55%

147.
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
148.
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
149.
Which of the following is considered an empirical formula?
a)

S2O4

b)
C6H12O6
c)
H2O
d)

C2H4

150.
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

151.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
152.
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
153.
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
154.

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)

HgCl2

b)

Hg3Cl

c)

Hg17Cl36

d)

HgCl

155.

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

a)

NO

b)

N2O4

c)

N2O3

d)

N2O5

156.

What is the empirical formula for P2O6?

a)

P2O6

b)

PO

c)

PO3

d)

P3O

157.

What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.

a)

K2SO4

b)

K8SO16

c)

K8S4O8

d)

K8S4O16

158.

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

159.

Determine the empirical formula of a compound containing 63.50 % silver, 8.25 % nitrogen, and the remainder oxygen.

a)

AgNO3

b)

Ag2NO3

c)

AgNO2

d)

Ag2N2O5

160.

What is the empirical formula for Si2F6?

a)

SiF

b)

Si2F6

c)

SiF3

d)

Si6F2

161.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
162.
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
163.

Which of the following could be a molecular formula with the empirical formula of CH2O?

a)

CH2O2

b)

CHO

c)

C3H5O3

d)

C2H4O2

164.

What is the empirical formula of Na2SO4?

a)

Na2SO4

b)

NaSO2

c)

Na2SO2

d)

NaSO8

165.

Match the following

a)

The actual number of atoms in a compound.

1.

MOLECULAR FORMULA definition

b)

The simplest reduced ratio of elements in a compound.

2.

EMPIRICAL FORMULA defintion

c)

N2O4N_2O_4

3.

MOLECULAR FORMULA example

d)

NO2NO_2

4.

EMPIRICAL FORMULA example

166.

MATCH THE EMPIRICAL AND MOLECULAR FORMULAS.

a)

N2O8N_2O_8

b)

NO4NO_4

1
2
1)
2)
167.

A compound is found to be 69.6% iron (Fe) and 30.4% oxygen (O) by mass. What is the empirical formula of the compound?

a)

FeO

b)

Fe2O3

c)

Fe3O4

d)

FeO2

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