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2nd Semester Final Review

Total questions: 108

Worksheet time: 2hrs 52mins

Name
Class
Date
1.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
2.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
3.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
4.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
5.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
6.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
7.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
8.
90 grams of sodium nitrate (NaNO3) are put into 100 grams of water and stirred. The final
mixture has a temperature of 20°C. About how many grams of the sodium nitrate dissolved?
a)
23
b)
73
c)
80
d)
88
9.
Students are asked to make statements about the solubility graph above. Which student does
the best job of communicating the general features of the graph?
a)
Most salts require 100 grams of water in order to dissolve completely.
b)
Table salt has the average solubility of all salts.
c)
The solubility of most salts increases with increasing temperature.
d)
Most curves show a decreasing slope as the temperature rises.
10.
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
11.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
12.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
13.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
14.

In the following, what is the unknown variable:

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm?

a)

P

b)

V

c)

n

d)

T

15.

What is the correct value for T in the following problem:

What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

a)

T = 0.23 K

b)

T = 293 K

c)

T = 4.2⁰C

d)

T = 20⁰C

16.

In the ideal gas law, P = ​ (a)   , V = ​ (b)   , n = ​ (c)   ,

R = ​​ (d)   , and T = ​ (e)  

Choose from the below words
pressure
volume
moles
gas law constant
temperature
17.

Under which conditions of temperature and pressure does carbon dioxide behave most like an ideal gas?

a)

A) Low temperature and low pressure

b)

B) Low temperature and high pressure

c)

C) High temperature and low pressure

d)

D) High temperature and high pressure

18.

A real gas differs from an ideal gas because the molecules of a real gas have

a)

A) Some volume and no attraction for each other

b)

B) Some volume and some attraction for each other

c)

C) No volume and no attraction for each other

d)

D) No volume and come attraction for each other

19.

Match the following units to their names.

a)

Pressure

1.

mmHg

b)

Volume

2.

L

c)

Temperature

3.

K

d)

Moles

4.

mol

20.

A real gas and ideal gas are similar at ​ (a)   pressures because the real gas particles ​ (b)   and have ​ (c)   collisions, like an ideal gas.

Choose from the below words
low
slow down
less
speed up
high
more
21.

A gas tank carrying 55L of Cl2 has a pressure of 2.6atm and a temperature of 289K. How many moles of chlorine gas are in the tank?

a)

6.03 mol

b)

0.55 mol

c)

1.45 mol

d)

0.75 mol

22.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
23.

Click the area of lowest pressure

A
B
C
D
24.

When Volume increases then Pressure must...

a)

Increase

b)

Decrease

25.

When Pressure increases then the Volume must...

a)

Increase

b)

decrease

26.

Which measurement can be identified by the unit K (Kelvin)?

a)

Temperature

b)

Volume

c)

Pressure

d)

Mass

27.

According to Charles Law, if Temperature of a gas increases Volume will also....

a)

Increases

b)

Decreases

c)

Stays the same

28.

If a balloon is placed in the freezer for several hours, then taken out and placed in a warm room, what would you expect to happen to the volume in the balloon?

a)

Volume would increase

b)

Volume would decrease

c)

Volume would not be effected

d)

Volume would briefly increase then decrease

29.

Your tire heats up as you drive it. This will result in...

a)

Pressure increasing

b)

Volume decreasing

c)

Pressure decreasing

d)

Temperature decreasing

30.

Two flasks are kept at the same temperature. Flask 1 has a pressure of 1.2atm, Flask 2 has a pressure of 1.5atm. Which of the following statements is true?

a)

Flask 1 has a smaller volume

b)

Flask 1 has a larger volume that Flask 2

c)

Flask 2 has a smaller volume

d)

Flask 1 has a higher temperature than Flask 2

31.

You blow up an inflatable for the pool. Everything seems great, but there is a hole in the inflatable and soon it is empty. This is an example of...

a)

Diffusion

b)

Effusion

c)

Partial Pressure

d)

Dalton's Law

32.

3 perfumes are sprayed across the room from you: Vanilla (112 g/mol), Fruity (145 g/mol) and Floral (125 g/mol). In what order would you smell the perfumes (first to last)?

a)

Vanilla, floral, fruity

b)

Floral, fruity, vanilla

c)

Fruity, floral, vanilla

d)

Vanilla, fruity, floral

33.

Select the temperature that would increase the kinetic energy of the particles the most.

a)

55oC

b)

341K

c)

70oC

d)

366K

34.

Select all that apply: If you doubled the pressure of a gas...

a)

The volume would decrease by half.

b)

The volume would double.

c)

The temperature would decrease by half.

d)

The temperature would double.

35.

Which energy diagram line represents the catalyzed reaction?

a)

The black line

b)

The red line

c)

It can not be determined

36.

D represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

37.

A represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

38.

B represents

a)

Potential Energy of Products

b)

Potential Energy of Reactants

c)

Change in Enthalpy

d)

Activation Energy

39.

Which of the following is true?

a)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of greater surface area.

b)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of lesser surface area.

c)

The reaction rate of the diagram on the right would be greater because there are more collisions that will happen because of greater surface area.

d)

The reaction rate of the diagram on the left would be greater because there are more collisions that will happen because of lesser surface area.

40.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

41.
In which experiment is the rate of reaction between hydrochloric acid and calcium carbonate slowest? 
a)
A
b)
B
c)
C
d)
D
42.
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
43.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
44.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
45.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
46.

When balancing an equation, you can NEVER change the...

a)

Coefficients

b)

Subscripts

47.

The small number after an element is called a...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

48.

The molecules and atoms on the right side of the arrow are called...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

49.

The molecules and atoms on the left side of the arrow are called...

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

50.

The large number in front of a molecule is called then....

a)

Reactants

b)

Products

c)

Coefficient

d)

Subscript

51.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

52.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

53.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

54.

This reaction is an example of....

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Single Replacement

e)

Double Replacement

55.

Baking a cake is a...

a)

Chemical change

b)

Physical change

56.

Mixing salt and water is a...

a)

Chemical change

b)

Physical change

57.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
58.

According to the collision theory, more collisions correspond to a:

a)

Faster reaction rate

b)

Slower reaction rate

c)

Constant reaction rate

d)

None of the above

59.
Which of the following IS a physical change?
a)
Getting a haircut
b)
Rusty metal
c)
sour milk
d)
A compound
60.
a copper penny turning greenish after a few years.
a)
Chemical Change
b)
Physical Change
61.
How many Al atoms are in this compound?         4Al2O3
a)
2
b)
8
c)
6
d)
4
62.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
63.

How do we make a dilution?

a)

Add more solute

b)

Remove solute

c)

Remove solvent

d)

Add more solvent

64.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

65.

How many moles of solute are present in 50.0 mL of 0.20M KNO3?

a)

10.0 moles solute

b)

0.05 moles solute

c)

1.00 moles solute

d)

0.01 moles solute

66.

How many mL of stock solution of 2M NaCl do you need to prepare 100 mL of 0.150M NaCl?

a)

7.5 mL

b)

15 mL

c)

1333 mL

d)

200 mL

67.

How many mL of 1.0M KBr solution would you need to prepare 250 mL of a 0.2M dilution?

a)

175 mL

b)

250 mL

c)

50 mL

d)

5 mL

68.

What would the molarity of a solution be if you took 10 mL of a 13M stock solution and made a 300 mL solution?

a)

390M

b)

230M

c)

0.43M

d)

0.26M

69.

You are adding a chlorine solution to a swimming pool. The stock solution of chlorine is 1000M. Your swimming pool (75,000 L) needs to be at a concentration of 0.1M. How much of the stock solution should you add?

a)

7500 L

b)

.75 L

c)

750 L

d)

7.5 L

70.

Balance this equation ​ (a)   N2 + ​ (b)   H2 --> ​ (c)   NH3

Choose from the below words
1
3
2
71.

Balance this equation. _CF4 + _Br2 → _CBr4 + _F2

a)

3,1,2,1

b)

1,2,1,2

c)

2,2,2,2

72.
Which of the following equations are correctly balanced?
a)

12CO2 +H2O --> C6H12O6 + O2

b)

CO2 + 9H2O --> C6H12O6 + O2

c)

CO2 + H2O --> 3C6H12O6 + O2

d)

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

73.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words
4
3
2
1
0
74.
What is the molar mass of C6H12O6?
a)

180.18 g/mol

b)

180.12 g/mol

c)

180.24 g/mol

d)

180.06 g/mol

75.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
76.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
77.
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
78.
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
79.

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

80.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.829 moles

81.

What is the mass of 4.98 x 1024 atoms of Zn?

a)

541 g

b)

8.27 g

c)

.122 g

d)

4.59 x 1046 g

82.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

83.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

84.

_____ reactions usually feel hot!

a)

endothermic

b)

exothermic

85.

Solid --> liquid --> gas is what type of reaction?

a)

endothermic

b)

exothermic

c)

catalytic

d)

inhibited

86.

gas --> liquid --> solid is what type of reaction?

a)

endothermic

b)

exothermic

c)

catalytic

d)

inhibited

87.

Endo means in or _______.

a)

absorbed

b)

released

88.

Exo means out or ________.

a)

absorbed

b)

released

89.

Ice cubes in your glass of soda melt.

a)

endothermic

b)

exothermic

90.

You freeze juice to make ice pops.

a)

exothermic

b)

endothermic

91.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
92.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
93.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

94.

How much activation energy is needed for this reaction?

a)

300 KJ

b)

500 KJ

c)

400 KJ

d)

100 KJ

95.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

96.

What kind of equation is this: 2KI + MgCl2 + 200KJ ----> 2KCl + MgI2

a)

Endothermic

b)

Exothermic

97.
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
98.

How can you tell this reaction is exothermic: MgO + CaS ----> CaO + MgS + 200 KJ

a)

Energy is written on the reactants side

b)

Energy is being released

c)

Energy is being absorbed

99.

if more heat energy is released in making bonds in the products than is taken in when breaking bonds in the reactants

a)

Exothermic

b)

Endothermic

c)

Exotermic

d)

Endotermic

100.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

101.

The diagram represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

a)

Heat energy flows from solid A to solid B. Solid A decreases in temperature

b)

Heat energy flows from solid A to solid B. Solid A increases in temperature

c)

Heat energy flows from solid B to solid A. Solid B decreases in temperature.

d)

Heat energy flows from solid B to solid A. Solid B increases in temperature.

102.
When you dropped a hot metal sample into room temperature water in the lab what happened?
a)
the heat from the metal traveled into the water
b)
the cool from the water traveled into the hot metal
c)
both of the other answers are correct
103.

Ice cream melting is an example of an __________ process.

a)

endothermic

b)

exothermic

104.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

105.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

106.

Which of the following is true?

a)

Energy transfers from hot to cold.

b)

Energy transfers from system to surroundings.

c)

Energy transfers from surroundings to the system.

d)

Energy transfers from cold to hot.

107.

When a bond is being formed, energy must be....

a)

absorbed

b)

released

108.

When a bond is being broken, energy must be....

a)

absorbed

b)

released

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