wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Chemistry Moles, % yield Empirical Formula

Total questions: 68

Worksheet time: 1hrs 21mins

Name
Class
Date
1.

What is the mole ratio from O2 to H20?

2H2 + O2 ---> 2H2O

a)

2:2

b)

1:2

c)

1:1

d)

3:1

2.

What is the mole ratio from Hydrogen to Oxygen?

2H2 + O2 ---> 2H2O

a)

2:2

b)

1:2

c)

2:1

d)

1:1

3.

How many moles of Oxygen are required to produce 13 moles of H2O?

2H2 + O2 ---> 2H2O

a)

6.5 moles O2

b)

35 moles O2

c)

3.5 moles O2

d)

3.25 moles O2

4.

How many moles of O2 are required to produce 20 grams of H2O?

2H2 + O2 ---> 2H2O

a)

20 moles O2

b)

.555 moles O2

c)

1.10 moles O2

d)

10 moles O2

5.

How many moles of O2 are required to produce 40 L of H2O?

2H2 + O2 ---> 2H2O

a)

40.0 moles O2

b)

1.76 moles O2

c)

.89 moles O2

d)

3.57 moles O2

6.

How many moles of O2 are required to produce 60 X 10^25 molecules of H2O?

2H2 + O2 ---> 2H2O

a)

1329 g O2

b)

5 g O2

c)

42 g O2

d)

986 g O2

7.

How many liters of O2 are required to produce 50L of H2O ?

2H2 + O2 -----> 2H2O

a)

2 L O2

b)

25L O2

c)

50 L O2

d)

100 L O2

8.

What is the molar mass of H2O?

a)

2.016 g/mole

b)

15.999 g/mole

c)

18.015g/mole

d)

33.006 g/mole

9.

What is the molar mass of H2?

a)

1.008 g/mole

b)

2.016 g/mole

c)

3.024 g/mole

d)

4.032 g/mole

10.

If you have 15 moles of compound A, you have ______ of compound A

Choose 2 answers

a)

336 L

b)

9.03 x 10^24 particles

c)

30 grams

d)

15 atoms

11.

IF 5 grams of compound A produces 20 grams of compound C, and 5 grams of compound B produces 10 grams of compound C, what is the limiting reactant?

a)

A

b)

B

c)

C

d)

D

12.

IF 5 grams of compound A produces 20 grams of compound C, and 5 grams of compound B produces 10 grams of compound C, what is the excess reactant?

a)

A

b)

B

c)

C

d)

D

13.

If you have an actual yield of 20 g and a theoretical yield of 40 g, what is the % yield?

a)

20%

b)

40%

c)

50%

d)

100%

14.

What is the difference between the actual and theoretical yield?

PIck 2

a)

Theoretical is calculated

b)

actual is calculated

c)

theoretical is determined in the lab

d)

actual is determined in the lab

15.

How much of a limiting reactant is used in a reaction?

a)

None

b)

Half

c)

All

d)

Depends

16.

What is an excess reactant?

a)

the reactant that has some left when the reaction stops

b)

reactant that is used up completely

c)

reactant that limits the amount of product

d)

reactant that produces the least amount of product

17.

If you are given grams of compound A and want to find grams of compound B, what will you need?

Pick 3

a)

Molar mass of A

b)

Molar mass of B

c)

1 mole = 22.4 L

d)

Mole ratios

18.

If you are given L of compound A and want grams of compound B, what will you need? Pick 3

a)

Molar mass of A

b)

Molar mass of B

c)

Mole ratios

d)

1 mole = 22.4 L

19.

If you are given g of compound A and want to find L of compound A, what will you need?

Pick 2

a)

Molar mass of A

b)

Molar mass of B

c)

Mole ratios

d)

1 mole = 22.4L

20.

If you are in L of compound A and want molecules of compound A what will you need?

Pick 2

a)

Molar mass of A

b)

Molar mass of B

c)

1 mole = 22.4 L

d)

1 mole = 6.02x10^23 molecules

21.

If you are given molecules of compound A and want moles of compound B, what will you need?

PIck 2

a)

Molar mass A

b)

Molar mass B

c)

1 mole = 6.02x10^23 molecules

d)

mole ratios

22.

If 234 g of CuCl2 are reacted with 320 g of NaNO3, how many grams of NaCl could be theoretically produced?

you have to balance this equation first

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

a)

220 g NaCl

b)

203 g NaCl

c)

440 g NaCl

d)

102 g NaCl

23.
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
24.
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
25.
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
26.
What does percent yield indicate?
a)
The amount of product we should get
b)
The efficiency of the lab
c)
The amount of product we actually got
d)
nothing
27.
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
28.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
29.
Percent yield = 100%
Theoretical yield = 88 grams
What is your actual yield?
a)
88 grams
b)
88%
c)
100 grams
d)
22%
30.
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
31.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
32.
Zn  +  CuCl​2​​  →  ZnCl​2​  ​+  Cu
How many moles of ZnCl2 will be produced from 23.0 g of Zn
a)
0.354 moles
b)
1495 moles
c)
47.76 g
33.
Zn  +  CuCl​2​​  →  ZnCl​2​  ​+  Cu
How many grams of ZnCl2 will be produced from 23.0 g of Zn
a)
0.354 moles
b)
1495 moles
c)
47.76 g
34.
Zn + 2HCl → ZnCl​2 ​​+ H​2​​
15 grams of HCl should theoretically produce 0.42 grams of H2. The reaction actually produced 0.15 grams of H2. What is the percent yield of H2?
a)
2.8%
b)
280%
c)
1%
d)
36%
35.

What is the formula for percent yield?

a)

ActualTheoretical×100\frac{Actual}{Theoretical}\times100

b)

TheoreticalActual×100\frac{Theoretical}{Actual}\times100

c)

Actual×Theoretical100\frac{Actual\times Theoretical}{100}

d)

100Actual×Theoretical\frac{100}{Actual\times Theoretical}

36.
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
37.
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
38.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
39.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

40.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
41.

The theoretical yield of a reaction is 237 grams, but the reaction actually yields 26 less grams than expected. What is the percent yield?

a)

17.6%

b)

82.4%

c)

89.0%

d)

121.3%

42.

If 5.2 grams of Mn(SO4)2 are actually formed in the lab, what is the percent yield?

The calculated number of grams for Mn(SO4)2 is 6.30 grams

a)

37%

b)

48%

c)

53%

d)

83%

43.

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

44.
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
45.

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)

58.83%

b)

308%

c)

6435%

d)

15.5

46.
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%
47.

What is the empirical formula of a substance with the molecular formula C2H4?

a)

C2H2

b)

C2H2

c)

C1H1

d)

CH2

48.

What is the empirical formula of a substance with the molecular formula NaCl?

a)

Na2Cl

b)

NaCl2

c)

NaCl

d)

Na2Cl2

49.

What is the empirical formula of a substance with the molecular formula X20Y15?

a)

X10Y15

b)

X5Y3

c)

X4Y3

d)

X20Y15

50.

What is the empirical formula of a substance with the molecular formula Se8F12?

a)

Se8F12

b)

Se2F3

c)

Se4F3

d)

SeF

51.

What is the empirical formula of this substance?

a)

C2H3

b)

CH3

c)

C2H6

d)

C2H2

52.

What is the empirical formula for hydrogen peroxide (H2O2)?

a)

H2O

b)

H2O2

c)

HO

d)

HO2

53.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
54.

Napthalene has the chemical formula C10H8. What would be the empirical formula?

a)

C10H8

b)

C5H4

c)

C20H16

d)

CH2

e)

C4H3

55.

Glucose has the formula C6H12O6. Maltose has the chemical formula C12H22O11. Do the have the same empirical formula?

a)

Yes

b)

No

56.

Which of these is NOT an empirical formula?

a)

CH2

b)

C2H5

c)

C6H4

d)

C3H7

e)

C5H17

57.

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

58.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

59.

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

60.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
61.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
62.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
63.
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
64.
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
65.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
66.

Determine the amount of moles in CuBr that are in 276.9 g of the compound.

a)

3.2 mol

b)

1.7 mol

c)

2.1 mol

d)

1.9 mol

67.

Determine the number of moles of Mg3P2 that are in 583 g of the compound.

a)

2.9 mol

b)

6.1 mol

c)

4.3 mol

d)

1.7 mol

68.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g

Similar Resources on Wayground

Chemistry Review 2024

71 questions

Chemistry Review 2024

quiz

Worksheet

•

10th Grade

Reacciones Químicas y sus ecuaciones 2°BGU UEMAAG

65 questions

Reacciones Químicas y sus ecuaciones 2°BGU UEMAAG

quiz

Worksheet

•

11th Grade

Periodic Law/Periodic Trends Practice Test

70 questions

Periodic Law/Periodic Trends Practice Test

quiz

Worksheet

•

10th Grade

Atoms and Periodic Table Review

63 questions

Atoms and Periodic Table Review

quiz

Worksheet

•

10th Grade

Unit 7 Chemical Reactions Review

72 questions

Unit 7 Chemical Reactions Review

quiz

Worksheet

•

10th Grade

Trace Review 2021

64 questions

Trace Review 2021

quiz

Worksheet

•

11th Grade

Balancing, Classifying, and Energy Test Review

66 questions

Balancing, Classifying, and Energy Test Review

quiz

Worksheet

•

9th - 12th Grade

2nd Semester Midterm Review

65 questions

2nd Semester Midterm Review

quiz

Worksheet

•

9th - 12th Grade