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The Mole Test Review

Total questions: 53

Worksheet time: 13hrs 15mins

Name
Class
Date
1.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

2.

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

3.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

4.

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

a)

atoms

b)

formula units

c)

ions

d)

molecules

5.

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

6.

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

7.

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)
8.

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

9.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

10.

How many atoms are in 1 mole of Iodine (I)?

a)

6.022 x 1023

b)

4.022 x 1023

c)

6.022 x 1025

d)

4.022 x 1025

11.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

12.

SELECT ALL CORRECT ANSWERS - The mole can be used to measure:

a)

The amount of atoms in an element

b)

The amount of molecules in a covalent substance

c)

The amount of formula units in an ionic compound

d)

The amount of mass an object has

13.

How many moles there are in 5.68 x 1024 atoms of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

14.

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)
15.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

16.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

17.

What is the correct equation to determine how many calcium ions (Ca2+) in 2 moles?

a)
b)
c)
d)

This cannot be determined as calcium is not bonded.

18.

What is the correct equation to calculate the number of moles in 3.13 x 1026 molecules of H2O2?

a)
b)
c)
d)
19.

What are the units for Avogadro's number?

a)

meters

b)

particles

c)

grams

d)

liters

20.

Find the mass of 11.37 mol of BaO. Round to the nearest whole number.

a)

1,354 g

b)

1,740 g

c)

17.40 g

d)

1,684 g

21.

Determine the number of moles of AlNO3 that are in 264 g of the compound.

a)

2.97 mol

b)

3.45 mol

c)

2.73 mol

d)

1.86 mol

22.

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

23.

Find the mass of 5.82 mol of MgCl2. Round to the nearest tenth.

a)

552.9 g

b)

436.8 g

c)

55.2 g

d)

555.9 g

24.

Determine the amount of moles of BaCl2 that are in 436 g of the compound.

a)

3.5 mol

b)

2.1 mol

c)

4.6 mol

d)

2.7 mol

25.

Find the mass of 3.8 mol of H2O. Round to the nearest tenth.

a)

57.9 g

b)

54.8 g

c)

68.4 g

d)

62.3 g

26.
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
27.
How to calculate molar mass of H2O?
a)
2+16=18
b)
1+16=17
c)
2+32=34
d)
1+31=32
28.

What is the molar mass of CO2?

a)

12 g/mol

b)

16 g/mol

c)

32 g/mol

d)

44 g/mol

29.

Find the percentage composition of Mg in Mg3(PO4)2.


a)

27.48% Mg

b)

43.11% Mg

c)

16.00% Mg

d)

12.63% Mg

30.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
31.
Which of the following is NOT needed to calculate percent composition?
a)
Mass of specific element
b)
Molar Mass
c)
Avogadro's Number
d)
Division
32.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

33.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
34.

What is the mass percentage of Carbon in Carbon dioxide (CO2)?

a)

27.27%

b)

42.86%

c)

72.73%

d)

72.72%

35.
What are the units in molar mass?
a)
grams
b)
moles
c)
moles/gram
d)
grams/mole
36.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
37.
Find the percentage composition of  Mg in Mg3(PO4)2.
   

a)
27.48% Mg
b)
43.11% Mg
c)
16.00% Mg
d)
12.63% Mg
38.
Find the molar mass of KCl
a)
36 g/mol
b)
78 g/mol
c)
74 g/mol
d)
178 g/mol
39.
Which of the following statements is NOT true?
a)
Molar mass is molecular mass
b)
Molar mass is the sum of the number of all atoms in one molecule
c)
Molar mass is the sum of the weight of all the atoms in the molecule
d)
You don't need atomic numbers when calculate molar mass
40.

The mass % of aluminum in aluminum sulfate Al2(SO4)3 is:

a)

12.93%

b)

45.70%

c)

7.89%

d)

35.94%

e)

15.77%

41.

The mass % of H in methane (CH4) is:

a)

75%

b)

92%

c)

25%

d)

4%

e)

6%

42.
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
43.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
44.
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
45.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
46.
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
47.
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
48.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
49.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
50.
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
51.
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 
52.
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
53.
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

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