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2022 Semester 2 Final Review

Total questions: 107

Worksheet time: 2hrs 11mins

Name
Class
Date
1.

Which would NOT increase the rate at which a sugar cube dissolves?

a)

Reducing the amount of solvent

b)

Crushing the sugar cube

c)

Stirring the solution

d)

Heating the solvent

2.

You can make a solute dissolve more quickly in a solvent by

a)

adding more solute.

b)

adding ice.

c)

heating the solvent.

d)

removing some solvent.

3.

A solution that contains all of the solute it can hold at a given temperature is

a)

diluted.

b)

saturated.

c)

supersaturated.

d)

unsaturated.

4.

The amount of solute that can be dissolved in a specific amount of solvent at a given temperature is its

a)

concentration.

b)

density.

c)

dilution.

d)

solubility.

5.

Three 10 g samples of sugar are represented below.


Sample A dissolves in water more slowly than sample B.

Sample B dissolves more slowly than sample C.

Which of the following best explains why sample A dissolves more slowly than the other two?

a)

It has the most volume.

b)

It has the smallest surface area.

c)

It has the largest number of sugar molecules.

d)

It has the fewest bonds between sugar modules.

6.

The solubility graph below shows the amounts of four substances that will dissolve in 100 grams of water at various water temperatures.


Which substance has 80 grams of solute dissolved in 100 grams of water at 50 C?

a)

Potassium Bromide

b)

Ammonium Chloride

c)

Potassium Chloride

d)

Lithium Hydroxide

7.

A solution that is able to dissolve additional solute is best described as

a)

supersaturated.

b)

concentrated.

c)

saturated

d)

unsaturated.

8.
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 
9.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
10.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
11.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
12.
The ___ is the thing being dissolved
a)
solute
b)
solvent
13.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

14.

If I add more chicken soup to this setup, what will happen to the pH?

a)

It will increase and get closer to 7

b)

It will decrease and get closer to 0

c)

It will stay the same and not change

15.

If I add more water to this setup, what will happen to the pH?

a)

It will increase and get closer to 7

b)

It will decrease and get closert to 0

c)

It will stay the same and not change

16.

Milk is a very weak acid. What might its pH value be?

a)

6.5

b)

7.8

c)

4.2

d)

12.2

17.

When an acid is dissolved in water, it turns red litmus paper blue.

a)

True

b)

False

18.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

19.

Which of the following is an acid?

a)

vinegar

b)

bleach

c)

sugar in water

d)

starch in water

e)

toothpaste in water

20.

Which of the following is a property of a base?

a)

bitter taste

b)

reacts with metals

c)

salty

d)

sour taste

21.

The pH value of an acid represents its __________ of positive ions in the solution

a)

amount

b)

concentration

c)

color

d)

charge

22.

Bases have many uses. They are mainly used to make

a)

cleaning products

b)

soaps

c)

concrete

d)

all of the answer choices

23.

The higher the concentration of negative (hydroxide) ions in the solution, the stronger the base is.

a)

True

b)

False

24.

The strongest bases have pH values close to

a)

0

b)

14

c)

7

d)

5

25.

Ocean water is only slightly basic. What might its pH value be?

a)

5

b)

8

c)

12

d)

2

26.

If the substance is neutral, what would the pH be?11

a)

3

b)

5

c)

7

d)

9

e)

11

27.
Explain what happens when a strong acid and a strong base are poured into the same container.
a)
they form separate layers
b)
they mix physically but not chemically
c)
they break apart into separate elements
d)
they react chemically to form a salt
28.
Which of the following is true about acids and bases?
a)
The lower the pH, the stronger the acid
b)
the higher the pH, the stronger the acid
c)
The lower the pH, the more neutral the acid
d)
The higher the pH, the weaker the base
29.
The flow of energy from an object at a higher temperature to an object at a lower temperature.
a)
heat
b)
temperature
c)
radiation
d)
conduction
30.
Heat transfer always goes from-
a)
Cold to Hot
b)
Hot to Cold
c)
Heat doesn't transfer
d)
Freezing to Cold
31.
"Stored energy" is another way of describing what energy type?
a)
Potential
b)
Electrical
c)
Kinetic
d)
Mechanical
32.
If your cup of hot chocolate is really hot that means it has a lot of this type of energy.
a)
Chemical
b)
Thermal
c)
Electrical
d)
Potential
33.
What form of energy is also described as "energy of motion"?
a)
Potential
b)
Mechanical
c)
Kinetic
d)
Electrical
34.
When plants convert the sun's energy into food, which type of energy is it?
a)
kinetic
b)
chemical
c)
thermal
d)
radiant
35.
What kind of energy does this device use?
a)
Chemical
b)
Electrical
c)
Thermal
d)
Chemical
36.
The glow sticks produce light for a short amount of time. The light from the glow stick is a conversion from what to what?
a)
thermal to light
b)
gravitational to potential
c)
radiant to electrical
d)
chemical to light
37.

Wind turbines and windmills convert what energy to another?

a)

Wind to Mechanical to electric

b)

Wind to Gravitational potential to electric

c)

Gravity to Mechanical to potential

d)

Solar to Thermal to sound

38.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
39.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

40.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
41.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
42.
A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true? 
a)
The temperature changed 
b)
It is an endothermic reaction
c)
It is an exothermic reaction 
d)
Two of the answers are correct 
43.
Have you ever eaten sherbet sweets candy? They fizz in your mouth and your tongue feels cold. Why do you think that is?
a)
It is an exothermic reaction
b)
It is an endothermic reaction
c)
It is made of ice
d)
It is dissolving your mouth
44.

What is an example of exothermic?

a)

firework

b)

ice pack

c)

coal

d)

wood

45.

Temperature is...

a)

A measure of the potential energy stored in a substance

b)

The same as heat

c)

A measure of the random motions of the molecules of a substance

46.

What tool do we use to measure kinetic energy of molecules?

a)

Thermometer

b)

Ruler

c)

Balance

d)

Magnifying Glass

47.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
48.
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
49.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

50.
The total energy of all the particles in a substance is called: 
a)
temperature
b)
thermal energy
c)
degrees
d)
mass
51.
What is a tool that measures the heat of chemical reactions?
a)
calorimeter
b)
 calorie
c)
Styrofoam™ cup
d)
none of these
52.
Calorimeters use insulating materials to:
a)
encourage affordable materials in science experiments in schools.
b)
preserve the heat of the environment outside the Styrofoam cup.
c)
prevent heat from escaping to the environment.
d)
keep the liquid inside the Styrofoam cup from overheating.
53.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
54.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

55.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

56.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
57.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
58.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
59.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
60.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
61.
Determine the initial temperature of a random gas when the initial volume is 2.2 L and it is cooled to 88K with a volume of 0.85 L. 
a)
0.029 K
b)
0.021 K
c)
227.76 K
d)
34 K
62.
What is the correct formula for Boyle's Law?
a)
V1/T1=V2/T2
b)
P1V1=P2V2
c)
P1/T1=P2/T2
d)
PV=nRT
63.
Which variable is held constant when using Boyle's Law?
a)
Temperature
b)
Pressure
c)
Volume
d)
number of moles
64.

What relationship can be interpreted from the diagram?

a)

As volume decreases, pressure decreases

b)

As pressure increases, volume increases

c)

As moles increase, temperature increases

d)

As pressure increases, volume decreases

65.

what is greenhouse effect

a)

the process of reflecting the heat from the back to the outer space.

b)

it is the process of trapping of heat from the sun by the greenhouse gases.

66.

An example of green house gas is:

a)

Oxigen

b)

Sulfure

c)

Chlorophyll

d)

Ozone

67.

Green House gases

a)

absorb the sun's radiation and trap heat

b)

are good for our health

c)

absorb gravity and keep us attached to Earth

d)

expulse radiation to the sun and prevent us from getting to warm

68.

Which of the following is not a green house gas?

a)

Ozone

b)

Carbon Dioxide

c)

Methane

d)

Helium

69.
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
70.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
71.
Gay-Lussac's law shows the directly proportional relationship between which two variables?
a)
pressure-temperature
b)
volume-temperature
c)
volume-pressure
d)
temperature-number of moles
72.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
73.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
74.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
75.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
76.
The ___________ the surface area of the reactants, the faster the reaction rate.
a)
larger 
b)
smaller
77.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
78.
Usually lowering the temperature will slow down a reaction.
a)
false
b)
true
79.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
80.
Exothermic reactions release heat to the surroundings.
a)
true
b)
false
81.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

82.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

83.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
84.
What does NOT happen when the temperature is increased?
a)
Particles collide more often
b)
Particles collide with more energy
c)
Particles move faster
d)
More particles collide in the correct orientation
85.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

86.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
87.
2A + 3B  <---->  2AB
The forward reaction points towards the __________.
a)
left
b)
right
c)
up
d)
down
88.
2A + 3B  <---->  2AB
The forward reaction forms the substance __________.
a)
A
b)
B
c)
AB
d)
A + B
89.
2A + 3B  <---->  2AB
The reverse reaction points towards the __________.
a)
left
b)
right
c)
up
d)
down
90.
2A + 3B  <---->  2AB
The reverse reaction forms the substance __________.
a)
A
b)
B
c)
AB
d)
A + B
91.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
92.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
93.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
94.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
95.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
96.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
both left and right
d)
neither left nor right
97.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
98.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse
99.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium will _______.
a)
shift left
b)
shift right
c)
not shift
100.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  _______ reaction will be favored.
a)
 the forward
b)
the reverse
c)
neither
101.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
102.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is decreased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
103.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is constant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
104.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
105.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
106.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
107.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product

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