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Worksheets

Finale Fun

Total questions: 131

Worksheet time: 33hrs 45mins

Name
Class
Date
1.
4.0 moles of H2O would have what mass?
a)
72 g
b)
23 g
c)
68 g
d)
4.5 g
2.
A mass of 6 g of Carbon contains
a)
1 mole of C
b)
2 moles of C
c)
0.5 moles of C
d)
72 moles of C
3.
How many moles are in 22 g of argon? 
a)
880 moles
b)
0.55 moles
c)
1.81 moles
d)
5 moles
4.
How many moles are in 9.8 grams of calcium? 
a)
0.2 moles
b)
4.1 moles
c)
1 mole
d)
392 moles
5.
How many grams are in 88.1 moles of magnesium?
a)
2141 g
b)
0.3 g
c)
30 g
d)
3.6 g
6.
How many moles are 98.3 grams of aluminum hydroxide, Al(OH)3?
a)
1.26 moles
b)
0.8 moles
c)
7,673.4 moles
d)
150 moles
7.
The number 6.02 x 1023 is ______.
a)
molar mass
b)
molecules
c)
Avogadro's number
d)
hydrate
8.
Which of the following has the same number of atoms as in 2 moles Carbon?
a)
All of them
b)
2 moles Mg
c)
2 moles K
d)
2 moles Al
9.

The law of conservation of mass says substances can neither be _______ nor ___________.

a)

Built; torn down

b)

Blended together; separated

c)

Created; destroyed

d)

Condensed; extracted

10.

Sodium and chlorine combine to form sodium chloride, or table salt. Sodium and chlorine are:

a)

Producers

b)

Products

c)

Reactionaries

d)

Reactants

11.

When sodium and chlorine combine to form sodium chloride, sodium chloride is the:

a)

Originator

b)

Reactant

c)

Product

d)

Produce

12.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
13.

What is the molar mass of fluorine gas, F2?

a)

18.998 g/mol

b)

38 g/mol

c)

9 g/mol

d)

18 g/mol

14.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
15.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
16.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
17.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
18.
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
19.
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
20.
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
21.
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
22.
The following is what type of reaction:
PbCl2 + AgNO3 → Pb(NO3)2 + AgCl
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
23.
The following is what type of reaction:
NH3 + HCl  → NH4Cl
a)
Synthesis
b)
Decomposition
c)
Single Replacement Replacement
d)
Double Replacement Replacement
24.
What type of chemical reaction is this?
Al(OH)3 → Al2O3  + H2O
a)
Decomposition
b)
Combustion
c)
Synthesis
d)
Single Replacement 
25.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Double Displacement
26.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis 
b)
Decomposition
c)
Single displacement
d)
Double displacement
27.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
28.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
29.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

30.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

31.
What is the molar mass of (NH4)2CO3 ?
a)
144 g
b)
138 g
c)
96 g
d)
78 g
32.
How can you figure out how particles (atoms) there are in 2 moles?
a)
2
b)
2 x (6.02 x 1023)
c)
2 x (atomic mass)
d)
2 ÷ (6.02 x 1023)
33.
The molar mass of an element is the mass of one ____ of the element.
a)
atom
b)
molecule
c)
mole
d)
gram
34.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

35.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

36.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
37.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
38.
The ___ is the thing being dissolved
a)
solute
b)
solvent
39.
What is the molarity of 1 mole of Ba+ in 2 L of water
a)
1 M
b)
2 M
c)
.5 M
d)
.25 M
40.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
41.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.07 gram
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
42.
Molarity is measured in
a)
moles per kg
b)
mols per L
c)
moles per kJ
d)
moles per mL
43.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

44.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
45.
Chocolate Milk
a)
Mixture
b)
Solution
46.
Where do you look to calculate the molar mass?
a)
avogadros number
b)
periodic table 
47.
A gas that has a pressure of 2 atm and a volume of 10 L.  What would be the new volume if the pressure was changed to 1 atm?
a)
P1/T1 = P2/T2
b)
P1V1 = P2V2
c)
V1/n1 = V2/n2
d)
PV = nRT
48.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
49.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
50.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
51.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
52.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
53.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
54.
What is 0 Kelvin known as
a)
No such thing
b)
Very cold
c)
Freezing point of Water
d)
Absolute Zero
55.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
56.
What is standard temperature?
a)
0K
b)
0oC
c)
173 K
d)
173.15 K
57.

Convert 175 K to °C.

a)

-98 °C

b)

79 K

c)

230.9 °C

d)

-48.2 °C

58.

Convert 100 °C to Kelvin.

a)

173 K

b)

373K

c)

273 K

d)

0 K

59.

Which temperature is equal to 20 K?

a)

-253°C

b)

-293°C

c)

253°C

d)

293°C

60.

Absolute Zero is which value:

a)

0 K

b)

0 °F

c)

0 °C

61.

If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?

a)

1.8 atm

b)

3.27 atm

c)

1.8 L

d)

3.27 atm

62.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
63.

How do you convert Kelvin to Celsius?

a)

Add 273

b)

Subtract 273

c)

You can't convert those

d)

They are the same thing

64.
Gas laws involve what three variables?
a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
65.

All of the following are temperature units except ______

a)

atm

b)

Kelvin

c)

Celsius

d)

Farenheit

66.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
67.
What is the variable for this number 122 K
a)
P
b)
T
c)
n
d)
V
68.
What is the variable for this number 1.5 mol
a)
P
b)
T
c)
n
d)
V
69.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
70.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
71.
Which has a bitter taste?
a)
Base
b)
Acid
c)
flagella
d)
cila
72.
Which has a pH below 7?
a)
Acid
b)
Base
73.
Which has a slippery texture?
a)
Acid
b)
Base
74.
Turns litmus red
a)
Acids
b)
Bases
c)
All
75.

What pH is the strongest base?

a)

1

b)

7

c)

4

d)

14

76.

What colour does a base turn red litmus paper?

a)

Red

b)

Blue

77.
Which of the following is most likely to be basic:
a)
Lemon juice
b)
Vinegar
c)
Laundry detergent
d)
Coke
78.
Which of these pH values would indicate that a solution is a weak base?
a)
4
b)
5.6
c)
8
d)
13
79.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
80.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
81.

A bronsted lowry base

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

82.

A bronsted lowry acid

a)

produces hydroxide ions in a solution

b)

is a proton donor

c)

produces hydrogen ions in a solution

d)

is a proton acceptor

83.

Identify the true statement about the following reaction:

F- + H2O --> HF +OH-

a)

H2O is a bronsted lowry base

b)

H2O is not an acid or base according to either model

c)

H2O is a bronsted lowry acid

d)

H2O is an arrhenius acid

84.

What is the conjugate base in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

85.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
86.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

87.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

88.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

89.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

90.

Water has a neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

91.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
92.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
93.

If the [H3O+] of a solution is 1 x 10-8 M the [OH-] is

a)

1.0 x 10-6 M

b)

1.0 x 106 M

c)

1.0 x 10-8 M

d)

1.0 x 108 M

94.

In what three ways does thermal energy transfer?

a)

radiation, fire, earth

b)

conduction, snow, radiation

c)

convection, conduction, radiation

d)

science, energy, motion

95.

The molecules in cold objects move

a)

slowly

b)

faster

c)

not at all

d)

out of this world

96.

The molecules in warm objects move

a)

slowly

b)

faster

c)

not at all

d)

out of this world

97.

Thermal energy transfer through touching is

a)

radiation

b)

conduction

c)

convection

d)

solar

98.

Warm air currents move upward from the earth. This is an example of

a)

convection

b)

conduction

c)

radiation

99.

Someone sits near a fire in a fireplace and becomes warmer. This is an example of:

a)

convection

b)

conduction

c)

radiation

100.
According to the picture, which one of the following best describes the order the states are shown?
a)
gas, liquid, solid
b)
solid, gas, liquid
c)
solid, plasma, liquid
d)
liquid, gas, solid
101.
A state of matter that has a definite volume and shape.
a)
solid
b)
liquid
c)
gas
d)
matter
102.
Solids have a definite _______________.
a)
smell
b)
shape
c)
picture
d)
sound
103.

Liquid matter takes the shape of _______.

a)

a gas

b)

water

c)

a pet

d)

Its container

104.

Measures how fast or how slow molecules are moving

a)

Density

b)

Temperature

c)

Heat

d)

All of them

105.
Heat always flows from a __________________ to a cooler object.
a)
warmer
b)
cooler
c)
coolest
d)
warmest
106.

Phase changes always involve changes in

a)

matter.

b)

space.

c)

color.

d)

energy.

107.
In heat transfer, heat always flows from the _______________ substance to the _______________ substance.
a)
Hotter to colder
b)
Colder to hotter
c)
Hotter to hotter
d)
Colder to colder
108.

What is the phase change of a solid to a liquid?

a)

freezing

b)

melting

c)

boiling

d)

condensation

109.
Change from gas to liquid...
a)
condensation
b)
evaporation
c)
expansion
d)
movement
110.

Change from Liquid to Solid is called ...

a)

fusion

b)

Freezing

c)

sublimation

d)

evaporation

111.

Change from liquid to gas is called....

a)

expansion

b)

evaporation

c)

condensation

d)

sublimation

112.

What happens to particles when energy is added (heated)?

a)

They speed up and spread out

b)

They slow down and compress

c)

They stop moving

d)

They move closer together and speed up

113.

Between which two points is the gas condensing?

a)

A <---- B

b)

B <---- C

c)

C <---- D

d)

D <---- E

e)

E <---- F

114.

Indefinite shape and indefinite volume:

a)

solid

b)

liquid

c)

gas

d)

plasma

e)

no such state

115.

Indefinite shape and definite volume:

a)

solid

b)

liquid

c)

gas

d)

plasma

e)

no such state

116.
The three types of nuclear radiation in increasing order of penetrating power are ____.  
a)
  alpha, beta, gamma 
b)
X ray, beta, gamma
c)
alpha, gamma, beta 
d)
X ray, gamma, beta 
117.
The most penetrating type of radiation is the ____.  
a)
alpha particle
b)
gamma ray
c)
beta particle
d)
uranium
118.
The type of radioactive particle that can be stopped by a sheet of paper is the ____.
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
uranium
119.
Radioactive materials have unstable...
a)
electrons
b)
protons
c)
nuclei
d)
neutrons
120.
A material that can stop gamma radiation is
a)
lead
b)
jello
c)
sunscreen
d)
wood
121.
After the third half-life, how much of the sample is left?
a)
1/2
b)
1/3
c)
1/16
d)
1/8
122.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
123.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
124.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
125.

The % of the parent isotope remaining after 1 Half Life.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

126.

The % of the parent isotope remaining after 2 Half Lives.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

127.

What is the Half Life of this isotope?

a)

3 days

b)

5 days

c)

8 days

d)

10 days

128.

Through relative dating, a geologist finds a fossil that is approximately 10,000 years old. Which radioactive element would geologist use to accurately calculate the fossils age?

a)

Gallium 67 with a half life of 78 hours

b)

Carbon-14 with a half-life of 5,700 years

c)

Plutonium-238 with a half-life of 88 years

d)

Iodine-129 with a half-life of 16 million years

129.
Nuclear power plants rely on which of the following reactions to generate energy?
a)
Fusion
b)
Half-life
c)
Fission
d)
Fusion or fission
130.
This is an example of...
a)
Fission  reaction
b)
Fusion reaction
c)
Decomposition reaction
d)
Combustion
131.
The time needed for half of a radioactive sample to decay is called its __________.
a)
decay period
b)
period
c)
transmutation time
d)
half-life