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Stoichiometry Quiz

Total questions: 126

Worksheet time: 11hrs 30mins

Name
Class
Date
1.

What do we call the mass of one mole?

a)

Atomic Number

b)

Molality

c)

Molarity

d)

Molar Mass

2.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

3.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

4.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

5.

What is the molar mass of Mg3N2?

a)

191.6 g/mol

b)

76.64 g/mol

c)

38.32 g/mol

d)

100.95 g/mol

6.

How many moles are in 4.5x1024 particles?

a)

0.747 particles

b)

0.747 mol

c)

2.71x1047 mol

d)

2.71x1047 particles

7.

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

8.
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
9.

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

10.

2H2 + O2 → 2H2O

How many moles of oxygen are consumed if 8 moles H2 are used?

a)

2

b)

4

c)

6

d)

8

11.

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

12.

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

13.

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%

14.

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

15.

What do we call the mass of one mole?

a)

Atomic Number

b)

Molality

c)

Molarity

d)

Molar Mass

16.

What is the molar mass of Potassium?

a)

19

b)

39.098 g/mole

c)

+1

d)

209 g/mole

17.

What is the molar mass of Bromine Chloride?

a)

79.90 g/mole

b)

150.80 g/mole

c)

150 Liters

d)

9.01 g/mole

18.

If you have one mole of elephants, how many moles of trunks and legs do you have?

a)

4 moles of trunks and 4 moles of legs

b)

1 mole of trunks and 1 mole of legs

c)

1 mole of trunks and 4 moles of legs

d)

2 moles of trunks and 1 mole of legs

19.

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)

Avogadro's Number

20.

In the balanced chemical equation to the left, how many moles of water are produced by reacting 1 mole of methane (CH4) with 2 moles of O2

a)

2 moles

b)

1 mole

c)

4 moles

d)

6.02 x 1023

21.

Balance this reaction: ____ LiNO3 + ____ MgF2 ----> ____ Mg(NO3)2 + ____ LiF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

22.

2 cups Flour + 1 cup oil + 1 cup buttermilk ---> 12 biscuits

How many cups of flour do I need to make 12 biscuits?

a)

1 cup

b)

2 cups

c)

4 cups

d)

I don't like biscuits

23.

2 cups Flour + 1 cup oil + 1 cup buttermilk ---> 12 biscuits

If I only have 1 cup of flour, how much oil and buttermilk will I need, and how many biscuits can I make?

a)

1 cup oil

1 cup buttermilk

12 biscuits

b)

1/2 cup oil

1/2 cup buttermilk

6 biscuits

c)

2 cups oil

1 cup buttermilk

24 biscuits

d)

I still don't like biscuits

24.

2H2 + O2 --> 2H2O

How many moles of O2 will be required to react with 6 moles of H2 ?

a)

1 mole O2

b)

4 moles O2

c)

3 moles O2

d)

8 moles O2

25.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of ammonia (NH3) to nitrogen?

N2 + 3H2 --> 2NH3

(a)  

26.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of oxygen to water produced?

2H2 + O2 --> 2H2O

(a)  

27.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of hydrogen to water produced?

2H2 + O2 --> 2H2O

(a)  

28.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of ammonia (NH3) to hydrogen?

N2 + 3H2 --> 2NH3

(a)  

29.

2H2 + O2 --> 2H2O


Based on the ratios in the chemical equation, if you have 4 mol of hydrogen, how many moles of water will be produced?

a)

1

b)

2

c)

4

d)

8

30.

3H2 + N2 --> 2NH3


Based on the ratios in the chemical equation, if you have 33 mol of hydrogen, how many moles of ammonia will be produced?

a)

11

b)

22

c)

33

d)

66

31.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

32.

What is the molar mass of Mg3N2?

a)

191.6 g/mol

b)

76.64 g/mol

c)

38.32 g/mol

d)

100.95 g/mol

33.

How many moles are in 4.5x1024 particles?

a)

0.747 particles

b)

0.747 mol

c)

2.71x1047 mol

d)

2.71x1047 particles

34.

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

35.
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
36.

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

37.

2H2 + O2 → 2H2O

How many moles of oxygen are consumed if 8 moles H2 are used?

a)

2

b)

4

c)

6

d)

8

38.

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

39.

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

40.

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%

41.

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

42.
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
43.
KNO3 --> KNO2 + O2
What coefficients are needed to balance the reaction?
a)
2, 2, 1
b)
2, 3, 2
c)
1, 2, 2
d)
1, 3, 1
44.

O2 + CS2 --> CO2 + SO2

What coefficient would go in front of the O2?

(a)  

45.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
46.
WO3 + H2 --> W + H2O
What coefficient goes in front of H2?
a)
1
b)
2
c)
3
d)
4
47.

You must convert (a)   to moles to complete a stoichiometry problem.

48.
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
49.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
50.
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
51.
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
52.
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
53.
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
54.
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
55.
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
56.
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
57.
A chemist interested in the efficiency of a chemical reaction would calculate the
a)
mole ratio
b)
rate of reaction
c)
percent yield
d)
energy released
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.
What is the molar mass of one molecule of Nitrogen N2?
a)
14.01 amu
b)
14.01 g
c)
28.02 g
d)
28.02 amu
60.
Calculate the molar mass of Mg(OH)2.
a)
33.2 g/mol
b)
41.3 g/mol
c)
86.9 g/mol
d)
58.3 g/mol
61.
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.
62.
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)
63.

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%

64.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
65.
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
66.

Stoichiometry is based on the law of conservation of

a)

charge

b)

mass

c)

reactants

d)

volume

e)

matter

67.

Do you feel comfortable with this information?

a)

No I don't have a clue.

b)

Yes, I got this.

c)

Are you crazy...I don't understand this.

d)

I kind of got it.

68.

True or False. You must convert grams to moles to do stoichiometry.

a)

True

b)

False

69.

The first step in stoichiometry is to

(a)  

70.
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
71.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
72.
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
73.
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
74.
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
75.
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
76.
Balance this equation
Zn+HCl-->ZnCl2 +H2
a)
Zn+HCl-->2ZnCl2 +H2
b)
Zn+HCl-->ZnCl2 +2H2
c)
Zn+2HCl-->ZnCl2 +H2
d)
2Zn+HCl-->ZnCl2 +H2
77.
Stoichiometry is based on the law of conservation of
a)
charge
b)
mass
c)
reactants
d)
volume
78.
How many molecules are in 1 mole of CO2?
a)
4.6 molecules
b)
4.6 grams
c)
6.02 x 10 23 molecules
d)
1.806x 10 24 atoms
79.
The first step in stoichiometry is to
a)
Determine a balanced equation
b)
convert grams to moles
c)
convert grams to liters
d)
use the mole ratio
80.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
a)
6 mol H2
b)
2 mol H2
c)
3 mol H2
d)
15 mol H2
81.
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
82.
Calculate the molar mass of Mg(OH)2.
a)
33 g/mol
b)
41 g/mol
c)
87 g/mol
d)
58 g/mol
83.
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
84.
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
85.
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
86.

What do we call the mass of one mole?

a)

Atomic Number

b)

Molality

c)

Molarity

d)

Molar Mass

87.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

88.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

89.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

90.

What is the molar mass of Mg3N2?

a)

191.6 g/mol

b)

76.64 g/mol

c)

38.32 g/mol

d)

100.95 g/mol

91.

How many moles are in 4.5x1024 particles?

a)

0.747 particles

b)

0.747 mol

c)

2.71x1047 mol

d)

2.71x1047 particles

92.

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

93.
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
94.

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

95.

2H2 + O2 → 2H2O

How many moles of oxygen are consumed if 8 moles H2 are used?

a)

2

b)

4

c)

6

d)

8

96.

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

97.

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

98.

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%

99.

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

100.

What do we call the mass of one mole?

a)

Atomic Number

b)

Molality

c)

Molarity

d)

Molar Mass

101.

What is the molar mass of Potassium?

a)

19

b)

39.098 g/mole

c)

+1

d)

209 g/mole

102.

What is the molar mass of Bromine Chloride?

a)

79.90 g/mole

b)

150.80 g/mole

c)

150 Liters

d)

9.01 g/mole

103.

If you have one mole of elephants, how many moles of trunks and legs do you have?

a)

4 moles of trunks and 4 moles of legs

b)

1 mole of trunks and 1 mole of legs

c)

1 mole of trunks and 4 moles of legs

d)

2 moles of trunks and 1 mole of legs

104.

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)

Avogadro's Number

105.

In the balanced chemical equation to the left, how many moles of water are produced by reacting 1 mole of methane (CH4) with 2 moles of O2

a)

2 moles

b)

1 mole

c)

4 moles

d)

6.02 x 1023

106.

Balance this reaction: ____ LiNO3 + ____ MgF2 ----> ____ Mg(NO3)2 + ____ LiF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

107.

2 cups Flour + 1 cup oil + 1 cup buttermilk ---> 12 biscuits

How many cups of flour do I need to make 12 biscuits?

a)

1 cup

b)

2 cups

c)

4 cups

d)

I don't like biscuits

108.

2 cups Flour + 1 cup oil + 1 cup buttermilk ---> 12 biscuits

If I only have 1 cup of flour, how much oil and buttermilk will I need, and how many biscuits can I make?

a)

1 cup oil

1 cup buttermilk

12 biscuits

b)

1/2 cup oil

1/2 cup buttermilk

6 biscuits

c)

2 cups oil

1 cup buttermilk

24 biscuits

d)

I still don't like biscuits

109.

2H2 + O2 --> 2H2O

How many moles of O2 will be required to react with 6 moles of H2 ?

a)

1 mole O2

b)

4 moles O2

c)

3 moles O2

d)

8 moles O2

110.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of ammonia (NH3) to nitrogen?

N2 + 3H2 --> 2NH3

(a)  

111.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of oxygen to water produced?

2H2 + O2 --> 2H2O

(a)  

112.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of hydrogen to water produced?

2H2 + O2 --> 2H2O

(a)  

113.

Write your answer as a ratio or a fraction: example 1/3

Based on the following chemical reaction, what is the ratio of ammonia (NH3) to hydrogen?

N2 + 3H2 --> 2NH3

(a)  

114.

2H2 + O2 --> 2H2O


Based on the ratios in the chemical equation, if you have 4 mol of hydrogen, how many moles of water will be produced?

a)

1

b)

2

c)

4

d)

8

115.

3H2 + N2 --> 2NH3


Based on the ratios in the chemical equation, if you have 33 mol of hydrogen, how many moles of ammonia will be produced?

a)

11

b)

22

c)

33

d)

66

116.

What is the mass of 54.3x1045molecules of BeO?

a)

3.27x1070 g

b)

9.01 x1022g

c)

2.25 x1024 g

d)

1.31 x1069g

117.

What is the molar mass of Mg3N2?

a)

191.6 g/mol

b)

76.64 g/mol

c)

38.32 g/mol

d)

100.95 g/mol

118.

How many moles are in 4.5x1024 particles?

a)

0.747 particles

b)

0.747 mol

c)

2.71x1047 mol

d)

2.71x1047 particles

119.

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

120.
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
121.

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

122.

2H2 + O2 → 2H2O

How many moles of oxygen are consumed if 8 moles H2 are used?

a)

2

b)

4

c)

6

d)

8

123.

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

124.

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

125.

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%

126.

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

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