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Mole, RMM, RFM, Molar Volume Calculation

Total questions: 100

Worksheet time: 3hrs 3mins

Name
Class
Date
1.
What is the definition of molar mass?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
2.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
3.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
4.
What is the definition for Avogadro's number?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
5.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
6.
Which represents the greatest mass of sulfur?
a)
1 gram of sulfur
b)
1 molecule of sulfur
c)
0.5 mole of sulfur
d)
6.02 x 1023 atoms of sulfur
7.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
8.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
9.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40 g
b)
80 g
c)
16 g
d)
32 g
10.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
11.
What is the molar mass of CO2?
a)
22.0 g/mol
b)
28.0 g/mol
c)
44.0 g/mol
d)
56.0 g/mol
12.
What is the molar mass of carbon?
a)
6.0 g/mol
b)
12.0 g/mol
c)
22.4 g/mol
d)
6.02 x 1023 g/mol
13.

A mole of potassium chloride, an ionic compound, contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

14.

An Avogadro's number of water molecules is equal to all EXCEPT _________.

a)

1 mole of water molecules

b)

2 moles of Hydrogen atoms and 1 mole of oxygen atoms

c)

18 grams of water

d)

18 molecules of water

15.

What is the molar mass of NaCl?

a)

58 g/mol

b)

28 g/mol

c)

12 g/mol

d)

6.02 x 1023

16.
If I have 6.02 x1023 molecules of CO2, what is the mass?
a)
44.0 g
b)
2.65 x1023 g
c)
1.37 x1022 g
d)
96.0 g
17.
What do we call the SI unit for amount of a substance?
a)
Avogadros number
b)
kilogram
c)
mole
d)
liter
18.

6.02 x 1023 is called

a)

Avocado number

b)

Standard form

c)

A mole

d)

Avogadro number

19.

Determine the mass of 0.2 mol of O2 gas

a)

3.2 g

b)

6.4 g

c)

32 g

d)

160 g

20.

The mass of 1 mol of O2 is

a)

8 g

b)

16 g

c)

24 g

d)

32 g

21.

How do you convert from grams to moles?

a)

Divide by the molar mass

b)

Multiply by the molar mass

c)

Divide by Avogadro's number

d)

Multiply by Avogadro's number

22.

How many atoms of copper in 65.0 g of copper(II) chloride?

a)

 2.91 ×1023 atoms2.91\ \times10^{23}\ atoms  

b)

 3.95 ×1023 atoms3.95\ \times10^{23}\ atoms  

c)

  5.81×1023 atoms5.81\times10^{23}\ atoms  

d)

  7.90×1023 atoms7.90\times10^{23}\ atoms  

23.

How many atoms of chlorine in 65.0 g of copper(II) chloride?

a)

2.91 ×1023 atoms2.91\ \times10^{23}\ atoms

b)

3.95 ×1023 atoms3.95\ \times10^{23}\ atoms

c)

5.81×1023 atoms5.81\times10^{23}\ atoms

d)

7.90×1023 atoms7.90\times10^{23}\ atoms

24.

If the molecular formula for compound Z is C8H18. What is the empirical formula?

a)

C8H18

b)

C4H8

c)

CH9

d)

C4H9

25.

If one Monster energy drink contains 0.16 g of caffeine, how many moles of caffeine do we consume when we drink 1 can? The chemical formula for caffeine is C8H10N4O2.

a)

194 mol

b)

1.57 ×10−3 mol1.57\ \times10^{-3}\ mol

c)


8.2474×10−4 mol8.2474\times10^{-4}\ mol

d)

3.14 ×10−3 mol3.14\ \times10^{-3\ }mol

26.

Caffeine has formula unit C8H10N4O2. Calculate the molar mass of caffeine.

a)

102

b)

24

c)

194

d)

124

27.

Acetone, C3H6O, is the main component of nail polish remover. Calculate the molar mass of acetone.

a)

42 g/mol

b)

10 g/mol

c)

32 g/mol

d)

58 g/mol

28.

Chalk is mostly made of calcium carbonate, CaCO3. If it took 48.6 g of chalk to write your name on the sidewalk, how many moles of calcium carbonate does your name contain?

a)

0.49 mol

b)

0.97 mol

c)

1.03 mol

d)

2.06 mol

29.

How many atoms are contained in 25 g of NaBr?

a)

6.54 x 1023 atoms

b)

3.27 x 1023 atoms

c)

2.93 x 1023 atoms

d)

1.46 x 1023 atoms

30.

How many molecules are in 2.00 moles of H2O?

a)

1.81x1024 molecules

b)

3.61x1024 molecules

c)

1.20x1024 molecules

d)

6.02x1023 molecules

31.

How many atoms are in 1.50 moles of Hg?

a)

9.03x1023 atoms

b)

6.02x1023 atoms

c)

4.82x1025 atoms

d)

1.21x1026 atoms

32.

How many grams are in 1.2 x 1024 molecules of CO?

a)

9.30 g

b)

55.81 g

c)

14.05 g

d)

0.50 g

33.

What is the volume of 5 moles of oxygen gas at room temperature?

a)

112 dm3

b)

112 cm3

c)

120 L

d)

120 mL

34.

Avogadro's number of representative particles is equal to one_____.

a)

molecule

b)

gram

c)

atom

d)

mole

35.

A container with a volume of 893 L contains how many moles of air at STP?

a)

2.5 x 10-2 mol

b)

39.9 mol

c)

22.4

d)

2.7 x 10-2 mol

36.

The volume of one mole of a substance is 24 L at RTP for all _____.

a)

gases

b)

solids

c)

compounds

d)

liquids

37.

Which volume will be occupied by a gas containing 6.02 x 1023 atoms at room temperature?

a)

1.0 L

b)

24 L

c)

22.4 L

d)

44.8 L

38.

The mass of 4.50 x 1022 Cu atoms is ___________

a)

4.75 g

b)

63.55 amu

c)

7.47 x 10-2 g

d)

7.47 x 10-2 amu

39.

What is the definition for Avogadro's number?

a)

number of grams per one mole of a substance

b)

whole number ratio that is a multiple of a chemical formula

c)

simplest, whole number ratio of a chemical formula

d)

6.02 x 1023 particles per one mole of a substance

40.

Sugar has formula unit C6H12O6 . Calculate the molar mass of sugar?

a)

96 g mol-1

b)

180 mol

c)

180 g mol-

d)

96 amu

41.

What do you think about this chapter (overall in two weeks)?

a)

Easy

b)

Intermediate

c)

Difficult

42.

How many moles are in 225g of CO?

a)

8.03 mole

b)

28.01 mole

c)

4.82x1024 mole

d)

7.50 mole

43.

How many moles are in 1.0g of NaCl ?

a)

0.181 mole

b)

6.0 x 1023 mole

c)

0.50 mole

d)

0.017 mole

44.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
45.
What is the definition of molar mass?
a)
number of grams per one mole of a substance
b)
whole number ratio that is a multiple of a chemical formula
c)
simplest, whole number ratio of a chemical formula
d)
6.02 x 10^23 particles per one mole of a substance
46.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
47.
How many moles are in 15g of lithium?
a)
104 mol
b)
2.2 mol
c)
0.46
48.
How many moles are in 22g of argon?
a)
0.55mol
b)
1.8mol
c)
8.8x102mol
49.
How many grams are in 2.4mol of sulfur?
a)
0.075g
b)
77g
c)
6.2x102g
50.
What is the molar mass of ammonium sulfate?
a)
114.12 g/mol
b)
132.17 g/mol
c)
209.27 g/mol
d)
2.32x105 g/mol
51.
How many moles are in 98.3 g of aluminium hydroxide?
a)
0.794 mol
b)
1.26 mol
c)
2.23 mol
d)
7.67x103 mol
52.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L 
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
53.
How many moles are there in 440g of carbon dioxide molecules?
a)
11
b)
10
c)
16
d)
0.25
54.
The number 6.02 x 1023 is called...
a)
Obama's number
b)
Bohr's number
c)
Trump's number
d)
Avogadro's number
55.
There are ______ number of molecules (atoms) of NaCl in one mole of NaCl?
a)
6.02 x 1023
b)
1 mole
c)
2
d)
Mr. Miller
56.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
57.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
58.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
59.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
60.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

61.

What is the Molar mass of the Baking Soda? (NaHCO3)

a)

84 gmol-1

b)

84 amu

c)

52 gmol-1

d)

52 amu

62.

What is the molar mass of (NH4)2CO3?

a)

96 gmol-1

b)

88 gmol-1

c)

40 gmol-1

d)

100 gmol-1

63.

What is the molar mass of water?

a)

18 gmol1-

b)

18

c)

20 gmol-1

d)

20

64.

What is the molar mass of magnesium hydroxide, Mg(OH)2?

a)

58 gmol-1

b)

24 gmol-1

c)

42 gmol-1

d)

60 gmol-1

65.

Which of the following is needed to determine the molar mass of a molecule?

a)

Types of elements in the molecule

b)

Quantity of elements in the molecule

c)

Mass of the elements in the molecule

d)

All are correct and needed.

66.
Molar volume of any gas at STP
a)
22.4 L
b)
2.24 L
c)
6.02 x 1023 L
d)
224 L
67.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
68.
A sample of carbon dioxide at STP is 0.50 L.  How many grams of carbon dioxide do we have?
a)
0.48 g
b)
0.49 g
c)
1.96 g
d)
0.98 g
69.

How many moles are in 225 g of CO?

a)

28.01 mol

b)

4.82 x 1024 mol

c)

6,302,25 mol

d)

8.0357 mol

70.

What is the formula to calculate the number of moles of a compound?

a)

Moles = mass/concentration

b)

Moles = molar mass/mass of sample

c)

Moles = mass/Mr

d)

Moles = distance/time

71.

What is Avogadro's constant?

a)

6.02 X 1023

b)

6.02 X 1022

c)

6.02 X 1032

d)

6.02

72.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
A unit of measurement to count particles
c)
based on the volume of a substance
d)
The number of atoms
73.
The unit for molar mass is
a)
g/mol
b)
mol/g
c)
grams
d)
moles
74.

What is the total number of molecules in 1.0 mole of CO2?

a)

1.5 x 1023

b)

12 x 1023

c)

3 x 1023

d)

6.02 x 1023

75.
The total number of sodium atoms in 46.0 grams is
a)
3.01 x 1023
b)
6.02 x 1023
c)
12 x 1023
d)
24 x 1023
76.
The relative atomic mass is the average mass of an atom compared to 
a)
the mass of a carbon-12 atom.
b)
1/12 the mass of a carbon-12 atom
c)
the mass of a hydrogen atom
d)
1/12 the mass of a hydrogen atom
77.
The relative molecular mass of a compound is equal to the sum of its
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
78.
What is the relative molecular mass of fluorine gas, F2?
a)
19
b)
38
c)
9
d)
18
79.
What is the unit of relative molecular mass?
a)
kilogram
b)
gram
c)
gram per mole (g/mol)
d)
no units
80.
The formula of a compound is M(OH)2. Given that the Mr of the compound is 98, calculate the Ar of M.
a)
32
b)
64
c)
81
d)
94
81.

Each element is defined by the number of

a)

Atoms

b)

Isotopes

c)

Neutrons

d)

Protons

e)

Nuclei.

82.

What is the relative formula mass of ammonium nitrate, NH4NO3 ?

[Relative atomic mass: N, 14; H, 1; O, 16]

a)

76

b)

79

c)

80

d)

90

83.
What is the atomic mass of magnesium?
a)
2
b)
4
c)
12
d)
24
84.
What is the relative formula mass of NaOH?
a)
20
b)
39
c)
40
d)
45
85.

Calculate the relative formula mass of

copper (ii) chloride, CuCl2


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

86.

Calculate the relative formula mass of

aluminium sulphate, Al2(SO4)3


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

87.

What is the relative atomic mass (Ar) of Carbon?

a)

6

b)

12

c)

18

d)

7

88.

What is the relative atomic mass (Ar) of Xenon (Xe)?

a)

54

b)

77

c)

131

d)

132

89.

What is the relative atomic mass (Ar) of Chlorine (Cl)?

a)

35.5

b)

17

c)

18.5

d)

0.5

90.

What is the relative molecular mass (Mr) of Hydrochloric Acid (HCl)?

a)

18

b)

34.5

c)

36.5

d)

35.1

91.

What is the volume at room conditions of a sample of ammonia gas, NH3 with the mass of 5.1 g?

a)

7.2 dm3

b)

12 dm3

c)

14.4 dm3

d)

18 dm3

92.

Which of the following is the correct chemical formula for copper(II) iodide?

a)

CuI

b)

Cu2l

c)

CuI2

d)

Cu2l2

93.

1.2 g of element Y combines with bromine to form 6 g of a compound with the empirical formula of YBr2. What is the relative atomic mass of element Y?

[Relative atomic mass: Br = 80]

a)

20

b)

36

c)

40

d)

56

94.

The following is a chemical equation:

H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + xH2O(l)

What is the value of x?

a)

1

b)

2

c)

3

d)

4

95.

The complete burning of ethanol is as follows.

C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)

What is the volume of oxygen gas needed at room conditions to burn 9.2 g of ethanol completely?

[Relative atomic mass: H = 1, C = 12, O = 16; Molar volume = 24 dm3 mol-1 at room conditions]

a)

4.8 dm3

b)

9.6 dm3

c)

14.4 dm3

d)

19.2 dm3

96.
Calculate the number of iron atoms in an iron nail.
a)
6.10 x 10^22
b)
3.36 x 10^25
c)
1.42 x 10^23
d)
6.023 x 10^25
97.
A mole of Neon contains
6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
98.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.0500 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
99.
Determine the molar mass for CCl4
a)
153.8 g/mol
b)
47.54 g/mol
c)
189.35 g/mol
d)
82.9 g/mol
100.

How many grams are in 1.2 x 1024 molecules of CO? (molar mass of CO = 28 g/mol)

a)

28.2 g

b)

55.8 g

c)

6.02 g

d)

1.2 g

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