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Moles Review Quiz

Total questions: 129

Worksheet time: 6hrs 23mins

Name
Class
Date
1.

A water molecule has the chemical formula H₂O. This means that the water molecule is made up of

a)

Two hydrogen atoms and one oxygen atom

b)

Two oxygen atoms and one hydrogen atom

c)

Two hydrogen atoms and two oxygen atoms

d)

Two molecules of water

2.

The atoms in a water molecule are held together by covalent bonds. This means that the bonded atoms

a)

Lose protons

b)

Lose electrons

c)

Share electrons

d)

Switch neutrons

3.

The water molecule is a polar molecule. A water molecule is polar because

a)

The electrons are shared equally

b)

Oxygen has a stronger attraction for electrons than hydrogen

c)

It is very cold

d)

Hydrogen atoms have a stronger attraction for electrons than oxygen

4.

The water molecule is

a)

Slightly negative near the hydrogen atoms and slightly positive near the oxygen atom

b)

Slightly positive in all areas of the molecule

c)

Slightly negative near the oxygen atom and slightly positive near the hydrogen atoms

d)

The same charge in all areas of the molecule

5.

Water molecules are attracted to each other because

a)

They are all positively charged

b)

Each water molecule has the same number of protons as electrons

c)

The positive area of one water molecule is attracted to the negative area of another

d)

All water molecules are neutral

6.

A paper clip can stay on the surface of water because of water's strong surface tension. Water's surface tension is mostly a result of

a)

Water's temperature

b)

The motion of water molecules

c)

The attraction of water molecules

d)

The impurities in the water

7.

Water cannot dissolve all substances that are made from ionic bonds. This is probably because

a)

Some water molecules are not as strong as others

b)

Water needs to be stirred to dissolve all ionic substances

c)

Some ionic bonds are too strong for the attractions of water molecules to pull them apart

d)

Water needs to be heated to dissolve all ionic substances

8.
Water beads up on the surface of a penny because of this property.
a)
Adhesion
b)
High Surface Tension
c)
Universal Solvent
d)
Changes in Density
9.

What type of intermolecular force does water experience?

a)

dispersion

b)

dipole

c)

covalent

d)

hydrogen "bond"

10.

Why does oil and water not mix together?

a)

because both compounds are polar

b)

because both compounds are nonpolar

c)

because water is polar and oil in nonpolar

d)

because water is nonpolar and oil in polar

11.

When an ionic compound dissolves in water, the ions _________________.

a)

remain together

b)

break apart

12.

Which type of compounds are typically electrolytes?

a)

ionic compounds

b)

metallic compounds

c)

molecular (covalent) compounds

13.

Which type of compounds are do not conduct electrical charge when dissolved?

a)

ionic compounds

b)

molecular (covalent) compounds

14.
The tightness across the surface of water that enables paper clips to float is ____________.
a)
adhesion
b)
capillary action
c)
surface tension
d)
polarity
15.

Why does ice stay at the top of oceans instead of sinking to the bottom? 

a)

Ice is colder than liquid water

b)

Ice is less dense than liquid water

c)

Ice is more dense than liquid water

d)

Ice is warmer than liquid water

16.

A water strider can skate along the top of a pond because....

a)

covalent bonds result in water cohesion (surface tension)

b)

hydrogen bonds result in water cohesion (surface tension)

c)

water striders have adapted to become lighter than water

d)

low surface tension of water

17.

Attractions between water molecules are called ....

a)

Covalent bonds

b)

Ionic bonds

c)

Polar bonds

d)

Hydrogen bonds

18.
Water is polar because...
a)
The unequal sharing of electrons gives the water molecule a slight negative charge near its oxygen atom and a slight positive charge near its hydrogen atoms.
b)
The molecule has two poles, at which the it is colder than other regions of the molecule.
c)
The unequal sharing of electrons gives the water molecule a slight negative charge near its hydrogen atoms and a slight positive charge near its oxygen atom.
d)
The water molecule is neutral.
19.
The fact that ice floats on liquid water is due to the fact that ........
a)
as water freezes, it expands and its density decreases.
b)
as water freezes, it takes up more hydrogen from the atmosphere, causing it to have a greater buoyancy.
c)
as water freezes, air becomes trapped between the hydrogen bonds of water molecules.
d)
as water freezes, it takes up more oxygen from the atmosphere, causing it to have a greater buoyancy.
20.

What kind of molecule is water?

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

d)

Metallic

21.

Which part of a water molecule has a Positive Charge?

a)

The Hydrogen

b)

The Oxygen

c)

The Top

d)

The Bottom

22.

Which part of a water molecule has a Negative Charge?

a)

The Hydrogen

b)

The Oxygen

c)

The Left

d)

The Right

23.
The _____is the part that gets dissolved. 
a)
solute 
b)
solvent 
c)
solution 
d)
Sacajawea 
24.
When one of the parts of the solution is water we call it _________. 
a)
water stuff 
b)
water mixture 
c)
aqua-man
d)
aqueous 
25.

This is the part of the solution that causes the dissolving to occur.

a)

solute

b)

solvent

c)

salt water

d)

the saturant

26.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
27.

Water dissolves __________ well.

a)

polar substances (like sugar)

b)

nonpolar substances (like oil)

c)

bricks

28.

Water doesn't dissolve __________ well.

a)

polar substances (like sugar)

b)

nonpolar substances (like oil)

c)

ice

29.

Loose ions that carry charge well (like in Gatorade) are called

a)

Powerade

b)

aqueous solutions

c)

electrolytes

30.

__________ electrolytes break apart completely and conduct electricity very well.

a)

Strong

b)

Weak

c)

Acid

31.

__________ electrolytes only break apart partly and conduct electricity a little bit.

a)

Strong

b)

Weak

c)

Acid

32.

Things that don't conduct electricity at all in a solution are called_______________.

a)

acid

b)

science

c)

nonelectrolytes

33.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
34.

If I dissolve carbon dioxide in water, what is the solvent?

a)

Carbon Dioxide

b)

There is no solvent

c)

Oxygen

d)

Water

35.

If I dissolve salt in water, what is the solvent?

a)

salt

b)

water

c)

salt & water

d)

none of the above

36.

At which temperature do KBr and KNO3 have the same solubility?

a)

60

b)

55

c)

50

d)

Never

37.

At 30'C, which substance has the lowest solubility?

a)

KNO3

b)

KBr

c)

NaCl

d)

Yb2(SO4)3

38.

At 80'C, KBr's solubility is:

a)

100g

b)

90g

c)

80g

d)

0g

39.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

40.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

60 g

d)

33 g

41.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
42.

What type of a solution is 180g sugar at 0ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

43.

What type of a solution is 180g sugar at 0ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

44.

A sample of a metal is 74% Aluminum. If the sample weighs 200 g, what is the mass of Aluminum in the sample?

a)

74 g

b)

200 g

c)

148 g

d)

100 g

45.

An element sample is 44% Zinc. If the sample has a mass of 5.0 g, what the mass of the Zinc in the sample?

a)

5.0 g

b)

220 g

c)

2.2 g

d)

There is no Zinc

46.
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
47.

What is the percentage of oxygen in carbon dioxide? (CO2)

a)
27.3%
b)
72.7%
c)
30%
d)
70%
48.
What is the percentage of chlorine in sodium chloride? (NaCl)
a)
60.7%
b)
39.3%
c)
60%
d)
40%
49.

What is the percentage of iron in iron(III)oxide (Fe2O3)?

a)
30%
b)
70%
c)
40%
d)
60%
50.

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

51.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
52.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
53.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
54.
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%
55.
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)
56.

Which element in the compound potassium cyanide, KCN, has a percent composition of 60.97%?

a)

K

b)

C

c)

N

d)

None of the above

57.

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

a)

29%

b)

43%

c)

57%

d)

73%

58.
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
59.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
60.
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
61.

How many molecules are in 2.5 mol of NaCl?

a)

1.5 x 1024 molecules

b)

1.5 molecules

c)

4.15 molecules

d)

1.5 x 1023 molecules

62.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
63.
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
64.
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
65.
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
66.

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

67.

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

68.
What is the empirical formula for C3H8
a)
CH
b)
C3H8
c)
C6H16
d)
CH2.7
69.
These kind of observation use your senses to observe results.
a)
Qualitative
b)
Quantitative
c)
Scientific
70.
These kind of observations are made using instruments such as rulers, balances and thermometers.
a)
Qualitative
b)
Quantitative
c)
Scientific
71.
It feels smooth.
a)
Qualitative 
b)
Quantitative
72.
The leaf is 5mm wide.
a)
Qualitative
b)
Quantitative
73.
10 ft = _________ in
a)
120
b)
0.83
c)
30
d)
12
74.
You know that 12 inches = 1 foot.  Convert 60 inches to feet.
a)
720 feet
b)
5 feet
c)
5 inches
d)
72 feet
75.

If Justin can type 408 words in 4 minutes, how many words can he type per minute? (Find the unit rate!)

a)

102 words per minute

b)

100 words per minute

c)

400 words per minute

d)

412 words per minute

76.

Which of the following statements regarding the mole is INCORRECT?

a)

A mole is a unit of quantity equal to 6.02 x 1023 particles.

b)

The number of particles in a mole is known as Avogadro’s number.

c)

A mole of particles of an element is numerically equal to the atomic mass of the element.

d)

none of the above

77.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

78.

What is a mole? - in chemistry -

a)

6.022 x 1023 particles of any substance

b)

A small burrowing animal

c)

A dark spot on your skin

d)

A spy

79.

Which of these elements has the highest molar mass?

a)

hydrogen

b)

iron

c)

carbonate

d)

cobalt

80.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

81.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

82.

How many grams are in 1.2 moles of neon (Ne)?

a)

0.059 grams

b)

7.2 x 1023 grams

c)

2.0 x 10-24 grams

d)

24 grams

83.

Converting moles to grams: How many grams are in 4 moles of sulfur (S)?

a)

256.24 grams

b)

128.12 grams

c)

64.06 grams

d)

512.48 grams

84.

Converting moles to grams: How many grams are in 2 moles of carbon (C)?

a)

48.04 grams

b)

24.02 grams

c)

36.04 grams

d)

12.01 grams

85.

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

86.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

87.

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

88.

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

89.

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.

90.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

91.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
92.
How many atoms are in 1 mole of NaCl? 
a)
6.02 x 1023
b)
58 
c)
11
d)
17
93.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
94.

5.11 x 1023 atoms of lithium (Li) is equal to how many moles?

a)

1.18 moles

b)

0.351 moles

c)

1.34 moles

d)

0.849 moles

95.

0.75 mole of copper (Cu) is equal to how many atoms?

a)

8.03 x 1023 atoms

b)

6.02 x 1023 atoms

c)

4.51 x 1023 atoms

d)

3.11 x 1023 atoms

96.

What is the mass of one mole of potassium (K)?

a)

19 grams

b)

39.10 grams

c)

30.97 grams

d)

38 grams

97.

0.50 moles of carbon (C) is equal to how many grams?

a)

6.0 grams

b)

12.0 grams

c)

8.0 grams

d)

14.0 grams

98.

36.0 g of beryllium (Be) contains how many moles?

a)

0.25 mol

b)

4.0 mol

c)

45 mol

d)

320 mol

99.

How many molecules are in 2.5 mol of Sodium Chloride?

a)

1.505x1023

b)

146

c)

4.15

d)

1.5x1024

100.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
101.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
102.

How many moles are in 1459 grams of Na?

a)

63.46 moles

b)

60.36 moles

c)

10 moles

d)

1 mole

103.

What is the molar mass of Al2S3?

a)

150.17 g/mol

b)

59.05 g/mol

c)

138.23 g/mol

d)

75.27 g/mol

104.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
105.

(a)   grams are in 2 moles of NaCl.

Choose from the below words
200 grams
50 grams
75 grams
116.88 grams
106.

Convert 50 grams of H2O to moles.

a)

2.78 moles

b)

5.0 moles

c)

25 moles

d)

0.5 moles

107.

How many moles are in 100 grams of CaCO3?

a)

0.999 moles

b)

1.999 moles

c)

2.5 moles

d)

0.5 moles

108.

Organize these units into the right categories

Categorize the following

Mol

Gram

Atoms

Nuclei

Molecules

Formula Units

Ions

Particles
Mole
Mass
109.

How is the molar mass of a compound calculated?

a)

By determining the temperature at which the compound changes state.

b)

By adding the atomic masses of all the atoms in a molecule of the compound.

c)

By measuring the volume of the compound at standard temperature and pressure.

d)

By weighing a single atom of the compound.

110.

What is the significance of Avogadro's number in relation to molar mass?

a)

It is the temperature at which a substance changes state.

b)

It is the mass of one mole of a substance.

c)

It is used to calculate the volume of a gas at standard temperature and pressure.

d)

It represents the number of atoms or molecules in one mole of a substance.

111.

How many grams are in 2.50 moles of sodium chloride?

a)
146.10 grams
b)
100.50 grams
c)
74.99 grams
d)
58.44 grams
112.

What is the molar mass of H₂O₂ used in the calculations?

a)

34.02 grams

b)

18.02 grams

c)

44.01 grams

d)

28.02 grams

113.

How many atoms are there in 1.25 grams of tungsten?

a)

3.75 x 1019 atoms

b)

1.00 x 1022 atoms

c)

2.50 x 1020 atoms

d)

4.09 x 1021 atoms

114.

How many grams are in 7.5 moles of LiCl?

a)

0.178 grams

b)

42 grams

c)

315 grams

d)

462 grams

115.

A mole of carbon =

a)

6.02 x 1023 carbon atoms

b)

12.011 carbon atoms

c)

one big ol' diamond

116.

Calculate the molar mass of boron trichloride

BCl3

a)

13 g/mol

b)

0.116 g/mol

c)

116 g/mol

d)

56 g/mol

117.
How many moles are in 32 grams of Oxygen (O)? 
a)
3
b)
2
c)
1
d)
4
118.

What is the molar mass when you have 4 moles of CO2?

a)

176 grams

b)

54 grams

c)

128 grams

d)

280 grams

119.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
120.

Calculate the moles in 12.7g of CaF2

a)

0.20 mol

b)

1,000.76 mol

c)

6.14 mol

d)

0.16 mol

121.

How many moles are in 100.0 g of dinitrogen oxide (N2O)?

a)

2.272 mol N2O

b)

6.25 mol N2O

c)

7.14 mol N2O

d)

44.013 mol N2O

122.

What is the mass of 2.50 mol of oxygen gas (O2)?

a)

40.0 g

b)

80.0 g

c)

16.0 g

d)

32.0 g

123.

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

124.

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

125.

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

126.

Find the mass of 3.6 mol of Au.

a)

843.6 g

b)

709.2 g

c)

435.9 g

d)

196.9 g

127.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
128.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
129.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.05 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5 moles

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125 questions

APES Unit 8 Review

quiz

Worksheet

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12th Grade

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134 questions

General Revision for Grade 9

quiz

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134 questions

Unit 3: Vet Science

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Worksheet

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129 questions

final exam practice

quiz

Worksheet

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10th Grade

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127 questions

Earth Science Final Exam Review

quiz

Worksheet

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12th Grade

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124 questions

Scientific Thinking Skills Review For Final

quiz

Worksheet

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6th - 12th Grade

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127 questions

Practice Questions

quiz

Worksheet

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9th Grade - University