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Worksheets

Semester 2 Exam Review Practice

Total questions: 180

Worksheet time: 15hrs 0mins

Name
Class
Date
1.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

2.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

3.

Is Fe2 a diatomic element?

a)

Yes

b)

No

4.

Is O2 a diatomic element?

a)

Yes

b)

No

5.

What are the coefficient used to balance the equation below?
__Ag2O →__ Ag +___O2

a)

2,4,1

b)

1,1,1

c)

2,1,2

d)

2,2,2

6.

Which problem is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

7.

Balance this equation.
_CH4 + _O2 --> _CO2 + _H2O

a)

1,2,1,1

b)

2,1,2,1

c)

1,2,1,2

d)

0,2,0,2

8.

Balance this equation.

__Mg + __Cl2 --> __MgCl2

a)

1, 2,1

b)

already balanced

c)

2,1,1

d)

1,1,2

9.

What type of reaction is Fe + Cl2 → FeCl3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

10.

What type of reaction is C2H2 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

11.

What type of reaction is Ag2O → Ag + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

12.

Select each compound that can be produced by combustion reactions. (more than 1 answer)

a)

Oxygen

b)

Carbon Dioxide

c)

Water

d)

Glucose

e)

Carbon

13.

Classify the following chemical reaction


BaCl2(aq) + K2CrO4(aq) --> BaCrO4(s) + 2KCl(aq)




a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

14.

Change from standard form to scientific notation: 12,000,000

a)

12.0  x  107

b)

0.12  x  107

c)

1.2  x  106

d)

1.2  x  107

15.

Change from standard form to scientific notation:  0.000398

a)

39.8  x  10-5

b)

3.98  x  10-5

c)

3.98  x  10-4

d)

39.8  x  10-6

16.

Change from standard form to scientific notation: 0.004078

a)

4.078  x  10-3

b)

4.078  x  103

c)

40.78  x  10-4

d)

.4078  x  10-2

17.

Try to change the number back to standard form:  6.79  x  104

a)

679,000

b)

6,790

c)

67,900

d)

6,790,000

18.

Which of the following is correct scientific notation?

a)

20.35 x 104

b)

.2035 x 104

c)

2035 4

d)

2.035 x104

19.

If the exponent is a positive number the original number was...

a)

a really big number.

b)

a really small number.

20.

If the exponent is a negative number the original number was...

a)

a really large number.

b)

a really small number.

21.

The SI unit for measuring volume is the __?__.

a)

meter (m)

b)

liter (L)

c)

cubic meter (m3)

d)

gram (g)

22.

The SI unit for measuring mass is the
 __?__.

a)

meter (m)

b)

liter (L)

c)

cubic meter (m3)

d)

kilogram (kg)

23.

The SI unit for time is the __?__.

a)

meter (m)

b)

liter (L)

c)

gram (g)

d)

second (s)

24.

Which SI unit is used to measure length?

a)

mol

b)

m

c)

kg

d)

m2

25.

This bullseye demonstrates...

a)

High Accuracy & High Precision

b)

High Accuracy & Low Precision

c)

Low Accuracy & High Precision

d)

Low Accuracy & Low Precision

26.

?

a)

High Accuracy & High Precision

b)

High Accuracy & Low Precision

c)

Low Accuracy & High Precision

d)

Low Accuracy & Low Precision

27.

This image is an example of...

a)

precision ONLY

b)

accuracy ONLY

c)

BOTH precision and accuracy

d)

NEITHER precision and accuracy 

28.

Measurements: 24.9, 25.2, 25.1, 24.8

True Value: 25.0

These measurements are…

a)

Accurate, but not precise

b)

Precise, but not accurate

c)

Both precise and accurate

d)

Neither precise nor accurate

29.

Measurements: 2.5, 14.5, 10.1, 45.3

True Value: 25.0

These measurements are…

a)

Accurate, but not precise

b)

Precise, but not accurate

c)

Both precise and accurate

d)

Neither precise nor accurate

30.

What is Avogadro's Number? (measures molecules and atoms)

a)

6.02 x 1023

b)

3.145

c)

it changes

d)

1

31.

The molar mass is found by

a)

adding the masses of all the atoms in the molecule.

b)

dividing the total mass of all the atoms in the molecule by 6.02 x 1023.

c)

multiplying the total mass of all the atoms in the molecule by 6.02 x 1023.

d)

dividing the total mass of all the atoms in the molecule by the total number of atoms.

32.

How many atoms are in 1.00 mole of Au?

a)

6.02 x 1023

b)

5.8 x 1024

c)

1.00 x1023

d)

79

33.

To solve these mole conversion problems, which of the following is CORRECT?

a)

multiply numbers on top and divide numbers on bottom

b)

add numbers on top and subtract numbers on bottom

c)

divide numbers on top and multiply numbers on bottom

d)

subtract numbers on top and add numbers on bottom

34.

The mole can be used to measure (SELECT ALL CORRECT ANSWERS)

a)

The amount of atoms

b)

The amount of molecules or compounds in a substance

c)

The amount of particles

d)

The amount of fission or fusion decay over time

35.

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

36.

What is the mass of one mole of silver?

a)

32.06 g

b)

107.87 g

c)

14.01 g

d)

22.99 g

37.

What are the units for molar mass?

a)

grams

b)

amu

c)

grams/mole

d)

liters

38.

Which chemical formula below indicates that you have three molecules of water ( H2OH_2O  )?

a)

3H2O3H_2O  

b)

H6O3H_6O_3  

c)

6HO6HO  

d)

H2OH_2O  

39.

Which chemical formula below matches the image shown here?

a)

2H2O2H_2O

b)

H4O2H_4O_2

c)

4H2O4H2O

d)

2HO2HO

40.

Which chemical formula below matches the image shown here?

a)

2H2O2H_2O

b)

H2O2H_2O_2

c)

4H2O4H2O

d)

2HO2HO

41.

What does the number 4 represent in 4NH3?

a)

Subscript

b)

Coefficient

42.

What does the number 3 represent in 4NH3?

a)

Subscript

b)

Coefficient

43.

How many iron atoms are in 
Fe(NO3)2

a)

1

b)

2

c)

3

d)

6

44.

How many hydrogen atoms are in this chemical formula: 

a)

4 hydrogen atoms

b)

1 hydrogen atom

c)

2 hydrogen atoms

d)

3 hydrogen atoms

45.

True or False. In the equation above there are a total of 2 hydrogen and 2 oxygen

a)

True

b)

False

46.

How many Magnesium atoms are in 10MgCl2?

a)

10

b)

5

c)

20

47.

What is a limiting reactant?

a)

the reactant that determines how much product can be made

b)

the reactant that is in excess

c)

the product that you can make the most of

d)

the amount of reactants that react with each other

48.

You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?

a)

bread

b)

jelly

c)

peanut butter

d)

sandwich

49.

The limiting reactant

a)

slows the reaction down

b)

is used up first

c)

is the reactant that is left over

d)

controls the speed of the reaction

50.

When does a chemical reaction stop?

a)

When the lab is finished

b)

When the excess reactant is used up

c)

When the limiting reactant is used up

d)

Chemical reactions never stop

51.

In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

4:3

d)

2:3

52.

Given the reaction: 4Al + 3O2 --> 2Al2O3

How many moles of Aluminum oxide are produced if you have 2 moles of Al?

a)

3 mole

b)

2 mole

c)

1 mole

d)

0.5 mole

53.

N2 + 3H2 → 2NH3

What is the mole ratio between Nitrogen and Ammonia in the above reaction?

a)

1 moles NH3 / 2 moles N2

b)

2 moles NH3 / 1 moles N2

c)

2 moles N2 / 3 moles NH3

d)

1 moles N2 / 3 moles NH3

54.

6CO2 + 6H2O --> C6H12O6 + 6O2

What is the total number of moles of water needed to produce 2.5 moles of C6H12O6?

a)

2.5

b)

6

c)

12

d)

15

55.

What is the SI Measurement for Amount of Substance?

a)

mole (mol)

b)

meter cubes (m3) liter (L)

c)

meter (m) centimeter (cm)

d)

joule (J) kJ

56.

What is the SI Measurement for Pressure?

a)

kelvin (K) *Celsius (*C)

b)

pascal (Pa) kilopascal (kPa)

c)

second (s)

d)

meter (m) centimeter (cm)

57.
Convert: 186.5 K to C
a)
-86.4 C
b)
-50 C
c)
-68.4 C
d)
180 K
58.

Convert 20.0oC to Kelvin.

a)

273 K

b)

298 K

c)

293 K

d)

20 K

59.

Convert 273K to oC

a)

546 oC

b)

-273 oC

c)

0 oC

d)

0 K

60.

Convert: -45.9 C to K:

a)

227.1 K

b)

400 K

c)

0 K

d)

373 K

61.

When a bottle is squeezed, the pressure increases and the volume __________.

a)

increases

b)

decreases

62.

The volume of a hot air balloon will __________ as the temperature is raised.

a)

increase

b)

decrease

63.

If the temperature of a can of hairspray is increased the pressure will _________ .

a)

increase

b)

decrease

64.

Gases best obey the ideal gas law at _____ .

a)

high temperatures and high pressures

b)

low temperatures and low pressures

c)

high temperatures and low pressures

d)

low temperatures and high pressures

65.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
66.
When Volume increases then Pressure must...
a)
Increase
b)
Decrease
67.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
68.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
69.

The volume of a sample of a gas at 273 oC is 200 liters. If the volume is decreased to 100 liters at constant pressure, what will be the new temperature of the gas?

a)

0 K

b)

546 K

c)

273 K

d)

100 K

70.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
71.
If 200 mL of a gas at 27°C is cooled to -33°C at a constant pressure, the volume will be
a)
250 mL
b)
204 mL
c)
196 mL
d)
160 mL
72.
Substance A is non-polar. If it dissolves in substance B, we can conclude that substance B is....
a)
Saturated
b)
Non-polar
c)
Polar
d)
A mixture
73.

Which statement is true?

a)

Solids will conduct electricity.

b)

Solutions (water with dissolved particles) will conduct electricity.

74.
An ______ is a compound that breaks apart in water, forming charged particles (ions) that can conduct electricity.
a)
electrolyte
b)
nonelectrolyte
c)
polar molecule
d)
non polar molecule
75.

Which TWO classes of materials will dissolve in water? (SELECT BOTH)

a)

acids & bases

b)

metals

c)

non-polar compounds

d)

electrolytes

76.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
77.

___________ refers to the amount of solute dissolved in a given amount per volume of solution

a)

Concentration

b)

Dilution

c)

Precipitation

d)

None of the above

78.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt


Solution 2:

500 mL of water

90 g of salt

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

79.

Which solution is more diluted?

Solution 1:

1000 mL of water

60g of salt


Solution 2:

500 mL of water

60 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally diluted

80.
When a solution is saturated:
a)
No additional material will dissolve in it
b)
You need to stir it more 
c)
Two materials have combined to create a clear liquid
d)
Crystals form 
81.

A solution with the maximum amount of solute completely dissolved.

a)

Saturated solution

b)

Unsaturated solution

c)

Supersaturated solution

82.

A solution with less than the maximum amount of solute completely dissolved.

a)

Saturated solution

b)

Unsaturated solution

c)

Supersaturated solution

83.

A solution with more than the maximum amount of solute completely dissolved.

a)

Saturated solution

b)

Unsaturated solution

c)

Supersaturated solution

84.

How does a solution become supersaturated?

a)

by pouring lots of solute in it then stirring.

b)

dissolve a little solute in it and stir.

c)

heat the solution to make it dissolve more solute and then cool it down.

d)

dissolve a small amount of solvent in it then heat it up.

85.

Which substance is MOST soluble at 0 ºC?

a)

KClO3

b)

NaNO3

c)

NaCl

d)

Ce2(SO4)3

86.

At what temperature can you fully dissolve 140g of NaNO3?

a)

62

b)

73

c)

81

d)

100

87.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

88.

What type of a solution is 60g NaCl at 80ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

89.

What type of a solution is 100g KNO3 at 70ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

90.

How would you describe a solution where the plotted point falls on the line on a solubility curve?

a)

unsaturated

b)

saturated

c)

supersaturated

91.

How would you describe a solution where the plotted point falls below the line on a solubility curve?

a)

unsaturated

b)

saturated

c)

supersaturated

92.

What type of solution is made when 80 g of NaNO3 is dissolved in 100 g of water at 10°C?

a)

saturated

b)

unsaturated

c)

supersaturated

93.

Which of theses is not an electrolyte?

a)

acids

b)

bases

c)

hydrocarbons

d)

ionic compounds

94.

In general, you cannot see through this mixture but you also cannot see any parts of it.

a)

solution

b)

colloid

c)

suspension

95.

In general, you usually cannot see through this type of mixture and you can notice layers or parts to it.

a)

solution

b)

colloid

c)

suspension

96.

Shaving Cream Foam

a)

Solution

b)

Suspension

c)

Colloid

97.

Muddy Water

a)

Solution

b)

Suspension

c)

Colloid

98.

Sugar Water

a)

Solution

b)

Suspension

c)

Colloid

99.

The particles in a suspension are _________ compared to the particles in a colloid.

a)

smaller

b)

larger

100.

Rate of solvation for a SOLID in a liquid ___________ as temperature increases.

a)

increases

b)

decreases

101.

Rate of solvation for a GAS in a liquid ___________ as temperature increases.

a)

increases

b)

decreases

102.

Rate of solvation for a SOLID in a liquid ___________ as the mixture is stirred.

a)

increases

b)

decreases

103.

Rate of solvation for a SOLID in a liquid ___________ as the solid is broken into smaller pieces.

a)

increases

b)

decreases

104.

Rate of solvation for a GAS in a liquid ___________ as pressure is decreased.

a)

increases

b)

decreases

105.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
106.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
107.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
108.

Pure water has a pH of 7. Pure water _______.

a)

is an acid

b)

is an base

c)

could be either an acid or a base

d)

is a neutral substance

109.

Vinegar has a pH of 2. Vinegar _______.

a)

is an acid

b)

is a base

c)

is a neutral substance

d)

could be either an acid or a base

110.

A solution of baking soda has a pH of 9. Baking soda _______.

a)

could be either an acid or a base

b)

is an acid

c)

is a neutral substance

d)

is a base

111.

What is the formula of hydrochloric acid?

a)
NaCl
b)
CO2
c)
H2O
d)
HCl
112.

What is the formula for nitric acid?

a)

CH3COOH

b)

HNO4

c)

NH3

d)

HNO3

113.

What is the formula for sulfuric acid?

a)

H2S

b)

H2SO4

c)

H2SO3

d)

H2SO5

114.

What is the formula for carbonic acid?

a)

H2C2O4

b)

H2O

c)

CO2

d)

H2CO3

115.

What is the formula for acetic acid?

a)

C3H6O3

b)

CH3COOH

c)

C2H4O

d)

C2H6O

116.

What is the formula for phosphoric acid?

a)

H2PO4

b)

H3PO3

c)

H4P2O7

d)

H3PO4

117.

What is the formula for sodium hydroxide?

a)
KOH
b)
NaCl
c)

Na(OH)2

d)
NaOH
118.

What is the formula for ammonia?

a)

NH2

b)

N2H4

c)

NH4+

d)

NH3

119.

What is the formula for calcium hydroxide?

a)

Ca(OH)3

b)

Ca(OH)2

c)

CaO2H2

d)

Ca(OH)4

120.

Phenolphthalein in an acid is ______________ .

a)

colorless

b)

pink

121.

Phenolphthalein in a base is ______________ .

a)

colorless

b)

pink

122.

Blue litmus paper turning red indicates the substance is ____________.

a)

acidic

b)

basic

c)

neutral

123.

Red litmus paper turning blue indicates the substance is ____________.

a)

acidic

b)

basic

c)

neutral

124.

An acid tastes _______ while a base tastes ______.

a)

soapy, sour

b)

sour, soapy

c)

salty, soapy

d)

sour, salty

125.

According to Bronsted-Lowry, what is the definition of an BASE?

a)

a substance that donates a hydrogen (H+) ion

b)

a substance that donates a hydroxide (OH-) ion

c)

a substance that accepts a hydrogen (H+) ion

d)

a substance that accepts a hydroxide (OH-) ion

126.

What colour does litmus paper turn when added to an acid?

a)

Blue

b)

Red

c)

Green

d)

Colourless

127.

Which type of acid/bases dissociate completely?

a)

strong

b)

weak

128.

How does the concentration of hydrogen ions affect the pH of a solution?

a)

Higher concentration of hydrogen ions leads to higher pH

b)

Higher concentration of hydrogen ions leads to lower pH

c)

Concentration of hydrogen ions has no effect on pH

d)

Lower concentration of hydrogen ions leads to higher pH

129.

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

130.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

131.
A compound that donates H+ ions is 
a)
A Bronsted-Lowry Acid
b)
An Arrhenius Acid
c)
A Bronsted-Lowry Base
d)
An Arrhenius Base
132.
Which of the following shows the correct conjugate acid base pair?
a)
HCI (acid) / H3O+ (conjugate base)
b)
HCI (acid) / CI- (conjugate base)
c)
HCI (base) / CI- (conjugate acid)
d)
HCI (base) / H3O+ (conjugate acid)
133.

In the equation below, what is the conjugate base?

HBr + H2O ↔ Br- + H3O+

a)

HBr

b)

H2O

c)

Br-

d)

H3O+

134.

NH3 + H2O --> NH4+ + OH-

What is NH4+ in this reaction?

a)

acid

b)

base

c)

conjugate acid

d)

conjugate base

135.

What is the conjugate base of HCl in the following reaction?

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

136.

What is the conjugate acid of PO43- following equation?

a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
137.

Given the reaction above, which compound is the acid?

a)

NH3

b)

HCl

c)

NH4+

d)

Cl-

138.

A solution with a pH of 2.0 has a hydrogen ion concentration ten times greater than a solution with a pH of:

a)

1.0

b)

3.0

c)

0.20

d)

20

139.
What are the products of the following reaction?
H2SO4  +  KOH  -->  
a)
HK  +  HSO4
b)
H2O  +  KSO4
c)
H2O  +  K2SO4
d)
H2  +  K2SO4
140.

Complete the following reaction:

H3PO4 + NaOH -->

a)

Na3PO4 + H2O

b)

Na +H2O

c)

Na3PO4 + H2

d)

Na3PO4 + H2O + CO2

141.

A __________ reaction is when an acid and a base are reacted together to produce water and a salt.

a)

Neutralization

b)

Volcanic

c)

Decomposition

d)

Single replacement

142.

If a solution has a [H+] of 9.3x10-11, what is the pH?

a)

10.0

b)

4.0

c)

3.5

d)

8.2

143.

If a solution has a [OH-] of 2.3x10-4, it must be a(n)...

a)

Acid

b)

Base

c)

Neutral

144.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
145.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
146.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
147.
If the [H+] of a solution is 6.8 x 10-9 mol/L the pH is
a)
8.17
b)
8.2
c)
9.99
d)
8.62
148.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
149.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

150.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
151.
The temperature of an unknown piece of metal with a mass of 30.00 g changes from 25.0 °C to 35.0 °C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?
a)
1.17 J/g°C
b)
-1.17 J/g°C
c)
0.857 J/g°C
d)
-0.857 J/g°C
152.

The SI units J/g°C measures

a)

Specific heat

b)

mass

c)

temperature

d)

heat energy

153.

An object with a higher specific heat requires _____ heat to raise its temperature.

a)

more

b)

less

154.

An _____________ releases heat so the container would feel ________.

a)

endothermic, warm

b)

endothermic, cold

c)

exothermic, warm

d)

exothermic, cold

155.

An _____________ reaction absorbs heat from the surroundings so the container would feel ________.

a)

endothermic, warm

b)

endothermic, cold

c)

exothermic, warm

d)

exothermic, cold

156.

When a hot object is put in cooler water, the temperature of the object _______ and the temperature of the water.

a)

rises, increases

b)

falls, increases

c)

rises, decreases

d)

falls, decreases

157.

The average kinetic energy of a substance's molecules ______ as it cools from 273K to 263K.

a)

increases

b)

decreases

158.

It takes longer for substance to _____ because the heat of vaporization is typically _______ than the heat of fusion.

a)

melt, higher

b)

boil, higher

c)

melt, lower

d)

boil, lower

159.

Gas particles are small compared to the volume thy occupy and in ______, ______ motion.

a)
fast, linear
b)
constant, random
c)
slow, circular
d)
steady, predictable
160.

The volume of empty space between gas particles is __________ so they experience ________ attraction or repulsion forces.

a)

large, a lot of

b)

small, very little

c)

large, very little

d)

small, a lot of

161.

According to the kinetic molecular theory (KMT), collisions between gas particles are elastic so kinetic energy is __________.

a)

gained

b)

lost

c)

conserved

162.

The average kinetic energy of a substance is expressed as a __________ .

a)
volume
b)
temperature
c)
pressure
d)
mass
163.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
164.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
165.
A substance that increases speed of chemical reaction without being being changed is called:
a)
Catalyst
b)
Acid
c)
Base
d)
pressure
166.
Activation energy is required to start a chemical reaction. What is activation energy?
a)
The energy needed for a reaction to occur
b)
The minimum amount of energy needed for a reaction to potentially occur
c)
The energy added by a catalyst
d)
The energy possessed by the products
167.

What is represented by interval C?

a)

Potential energy of the reactants

b)

Potential energy of the products

c)

Activation Energy

d)

Heat of reaction

168.

What does A + B represent?

a)

Reactants

b)

Products

c)

Activation Energy

d)

Heat of reaction

169.

Is this reaction endothermic or exothermic?

a)

Endothermic

b)

Exothermic

170.
In an exothermic reaction the products have
a)
more energy than the reactants
b)
the same energy as the reactants
c)
less energy than the reactants
d)
no energy
171.
In an endothermic reaction the products have 
a)
more energy than the reactants
b)
less energy than the reactants
c)
the same energy as the reactants
d)
no energy
172.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
173.

What part of the heating curve would ice be located at?

a)

A

b)

B

c)

C

d)

D

e)

E

174.

What part of the heating curve would liquid be located at?

a)

A

b)

B

c)

C

d)

D

e)

E

175.

What part of the heating curve would steam be located at?

a)

A

b)

B

c)

C

d)

D

e)

E

176.

Where are the phase changes located in the heating curve?

a)

A

b)

B

c)

C

d)

D

e)

E

177.

What happens to the kinetic energy of the substance in sections B and D?

a)

KE increases

b)

KE decreases

c)

KE stays the same

d)

The answer cannot be determined with the information provided.

178.

What happens to the kinetic energy of the substance in sections A, C and E?

a)

KE increases

b)

KE decreases

c)

KE stays the same

d)

The answer cannot be determined with the information provided.

179.

A catalyst _______ a reaction by _______ the activation energy

a)

speeds up, raising

b)

speeds up, lowering

c)

slows down, raising

d)

slows down, lowering

180.

An inhibitor _______ a reaction by _______ the activation energy

a)

speeds up, raising

b)

speeds up, lowering

c)

slows down, raising

d)

slows down, lowering

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