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PRACTICE - Semester 2 Final Exam PRACTICE Questions

Total questions: 145

Worksheet time: 5hrs 34mins

Name
Class
Date
1.

Predict the precipitate when you mix silver nitrate and sodium chloride:

a)

AgNO3

b)

No precipitate

c)

AgCl

d)

NaNO3

2.

When you mix barium nitrate and sodium sulfate

a)

BaSO4

b)

NaNO3

c)

No precipitate

d)

BaNO3

3.

When you mix magnesium nitrate and sodium hydroxide

a)

No precipitate

b)

NaOH

c)

NaNO3

d)

Mg(OH)2

4.

When you mix lithium iodide and silver nitrate

a)

AgI

b)

LiNO3

c)

AgCl

d)

All of the above

5.

AB (aq) + CD (aq) → AD (aq) + CB(s)


Which substance is the precipitate in the reaction above?

a)

AB

b)

CD

c)

AD

d)

CB

6.

Which of the following salts are not aqueous?

a)

NaBr

b)

Ca(NO3)2

c)

AgCl

d)

(NH4)2CO3

7.

Predict the products of a reaction between

Pb(NO3)2 (aq) + Na2(SO4) (aq)

a)

PbSO4 (aq) +NaNO3 (aq)

b)

PbSO4 (s) +NaNO3 (aq)

c)

Pb(SO4)(aq) +Na2(NO3) (aq)

d)

PbSO4 (s) +Na2(NO3)2 (aq)

8.

Which term is incorrectly described?

a)

aqueous = dissolved in water to make a water solution

b)

insoluble = unable to dissolve

c)

precipitate = made from water

d)

soluble = able to dissolve

9.

When solutions of two ionic compounds are combined and a solid forms, the process is called

a)

hydration

b)

solvation

c)

dissociation

d)

precipitation

10.

Which of these results in the formation of a precipitate?

a)

AgNO3(aq) + NaOH(aq)→

b)

Ba(NO3)2(aq) + CaCl2(aq)→

c)

NaNO3(aq) + KOH(aq)→

d)

More than one of these form precipitates

11.

Which of the following best describes a precipitate?

a)

an insoluble solid

b)

a soluble solid

c)

a soluble gas

d)

an insoluble liquid

12.
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)
13.
Which of the following shows the correct conjugate acid base pair?
a)
H2O (base) / H3O+ (conjugate acid)
b)
H2O (acid) / CH3COO- (conjugate base)
c)
CH3COOH (acid) / H3O+ (conjugate base)
d)
CH3COOH (base) / CH3COO- (conjugate acid)
14.
Which of the following shows the correct conjugate acid base pair?
a)
SO32-(base) / HSO3- (conjugate base)
b)
HPO42- (acid) / HSO3-(conjugate base)
c)
SO32-(acid) / HSO3- (conjugate base)
d)
HPO42- (acid) / PO43-(conjugate base)
15.

An acid has a pH

a)

higher than 7

b)

lower than 7

c)

7

d)

greater than 14

16.
What is the pH of water? 
a)
1
b)
3
c)
7
d)
10
17.
Accepts a proton (H+ hydrogen ion) 
a)
Lewis Base
b)
Arrhenius Base
c)
Bronstead Lowry Base
d)
Lewis Acid 
18.
Forms a OH- hydroxide ion
a)
Lewis Base
b)
Arrhenius Base
c)
Bronsted Lowry Base
d)
Bronsted Lowry Acid
19.
Which of the following is transferred between a conjugate acid-base pair?
a)
An Electron
b)
A OH- ion
c)
A Proton
d)
A Neutron
20.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

21.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

22.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
23.

Bases have a pH of

a)

7

b)

Less than 7

c)

More than 7

24.

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

25.

Choose the correct statements about HI based on the following reaction (select all that apply):

HI + H2O --> I- + H3O+

a)

HI is an arrhenius acid

b)

HI is an arrhenius base

c)

HI is a bronsted lowry acid

d)

HI is a bronsted lowry base

26.

Which of the following show an acid and its conjugate base pair (in that order)

a)

H2SO4, SO42-

b)

OH-, H2O

c)

NH4+, H2O

d)

H2CO3, HCO3-

27.
In the reaction HCl + H2O --> H3O+ + Cl-, what is the conjugate acid?
a)
HCl
b)
H2O
c)
H3O+
d)
Cl-
28.
What is the conjugate acid to NO3- ? (HINT...acids contain what ion?)
a)
HNO3
b)
OH-
c)
H+
d)
NO3-2
29.

Which solution is the most concentrated:

a)

Solution A

b)

Solution B

c)

Solution C

d)

They all have the same concentration

30.

Which solution is the most concentrated:

a)

Solution A

b)

Solution B

c)

Solution C

d)

They all have the same concentration

31.

Which solution is the least concentrated:

a)

Solution A

b)

Solution B

c)

Solution C

d)

They all have the same concentration

32.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
33.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
34.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
35.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
36.
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
37.
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
38.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
39.

The term molar which is used to describe a solution's concentration, is written as?

a)

M

b)

mol

c)

g

d)

g/L

40.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
41.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
42.

If you have 34 mL of a 0.5 M NaBr solution, what will the concentration be if 56 mL of water is added to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

43.

The units "M" can also be written as:

a)

mol/L

b)

moles

c)

g/L

d)

g/mol

44.

40 grams of NaOH = ________ moles

a)

1

b)

2

c)

160

d)

1600

45.

If 1 mole of solute is dissolved in 1 liter of water, what is the molarity?

a)

2M

b)

.5M

c)

1M

d)

It can't be determined unless you know the solute

46.

Which segment of the graph represents a time when both the solid and liquid phases are present?

a)

AB

b)

BC

c)

DE

d)

EF

47.

Which segment of the graph represents a time when both the liquid and gas phases are present?

a)

AB

b)

BC

c)

DE

d)

EF

48.

Which states of matter are present between line segment BC?

a)

Solid and Liquid

b)

Solid and Gas

c)

Liquid and Gas

d)

Solid only

49.

Which segment of the graph represents both melting and freezing?

a)

AB

b)

BC

c)

DE

d)

EF

50.

Which segment of the graph represents both vaporization and condensation?

a)

AB

b)

BC

c)

DE

d)

EF

51.

What is the melting point of the substance?

a)

-60 oC

b)

60 oC

c)

- 100 oC

d)

100 oC

52.

What is the boiling point of the substance?

a)

-60 oC

b)

60 oC

c)

- 100 oC

d)

100 oC

53.

Which will heat up faster?

a)

copper

b)

granite

c)

iron

d)

basalt

54.

Which will heat up slower?

a)

water

b)

lead

c)

granite

d)

iron

55.

Which of the following best explains why the sand at the beach is hotter than the water?

a)

Sand has a higher specific heat than water.

b)

Sand has a lower specific heat than water.

c)

There is more water than sand at the beach.

d)

There is more sand than water at the beach.

56.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
57.
How does heat flow?
a)
Always from cold to warm
b)
Always from warm to cold
c)
Both warm to cold & cold to warm
d)
It depends on the temperature
58.

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

59.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
60.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
61.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
62.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

63.

IF we are using Boyles' law and our Pressure goes UP, what must our volume do?

a)

Go UP

b)

Go DOWN

c)

Stay the same

d)

Wrong law.

64.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
65.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
66.

I have added 15 L of air to a balloon at sea level (1.0 atm). If I take the balloon with me to Denver, where the air pressure is 0.85 atm, what will the new volume of the balloon be?

a)

24 L

b)

18 L

c)

32 L

d)

15 L

67.
This graph is an example of two variables that are:
a)
directly proportional
b)
inversely proportional
c)
Straight line
d)
No relation
68.

Which best explains why increasing the pressure on a gas decreases the volume of the gas sample?

a)

Increasing the pressure causes the gas particles to hit the container walls more often.

b)

Increasing the pressure on a gas sample moves the gas particles closer together.

c)

Increasing the pressure on a gas sample causes the kinetic energy to increase.

69.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
70.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
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.
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
73.
The volume of a gas at 25ο C is 3.8 L.  What will be the volume of that gas at 57 ο C if the pressure is held constant?
a)
8.66 L
b)
4.21 L
c)
6.34 L
d)
3.46 L
74.
A sample of oxygen gas in a closed system has a volume of 200 milliliters at 600 K. If the pressure is held constant and the temperature is lowered to 300 K, the new volume of the gas will be -
a)
400 milliliters.
b)
300 milliliters.
c)
100 milliliters.
d)
200 milliliters.
75.

Define: Calorimeter

a)

In any chemical or physical process, energy is neither created nor destroyed.

b)

the heat absorbed or released by a chemical reaction

c)

a process that loses heat to the surroundings

d)

a device used to measure the amount of heat absorbed or released during chemical or physical change

76.

Define: Specific Heat

a)

the amount of heat that must be added to one unit of mass of the substance in order to cause an increase of one unit in temperature

b)

a process where energy is absorbed by the system from the surroundings

c)

the quantity of heat that raises the temperature of 1 g of pure water 1°C

d)

a process that loses heat to the surroundings

77.

Define: Heat

a)

a process that loses heat to the surroundings

b)

a device used to measure the amount of heat absorbed or released during chemical or physical change

c)

the amount of energy that is transferred from one system to its surroundings because of a temperature difference

d)

the heat absorbed or released by a chemical reaction

78.

Define: Calorie

a)


a process that loses heat to the surroundings

b)

the quantity of heat that raises the temperature of 1 g of pure water 1°C

c)

the heat absorbed or released by a chemical reaction

d)

the amount of energy that is transferred from one system to its surroundings because of a temperature difference

79.

If a 235 g sample of steam at 135 C is cooled to 112C, find the change in heat content of the system.

a)

10.8 kJ

b)

22.6 kJ

c)

-10.8 kJ

d)

-22.6 kJ

80.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

81.

_____ reactions usually feel hot!

a)

endothermic

b)

exothermic

82.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

83.

Endo means in or _______.

a)

absorbed

b)

released

84.

Exo means out or ________.

a)

absorbed

b)

released

85.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
bubbles of gas appear
d)
dissolving
86.
After you mix two substances together, a new substance forms.  This is an example of:
 
a)
 Physical Change
b)
 Chemical Change
87.
Is photosenthysis an Exothermic or an Endothermic reaction?
a)
Endothermic
b)
Exothermic
88.

Fireworks are an example of

a)

exothermic

b)

endothermic

c)

both

d)

none

89.

A melting ice cube is an example of

a)

exothermic

b)

endothermic

c)

none

d)

both

90.
2NaClO3 (s) → 2NaCl (s) + 3O2 (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
91.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
92.
Fe2O3 + 3H2 → 2Fe + 3H2O
About how many grams of H2O will be produced from 150 grams of Fe2O3? 
a)
50 grams H2O
b)
60 grams H2O
c)
5000 grams H2O
d)
6000 grams H2O
93.
Given the following reaction, 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
94.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
95.
How do I move from grams to moles
a)
multiply by molar mass
b)
divide by molar mass
c)
multiply by Avo number
d)
divided by Avo number
96.
Use the following equation:
2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide?
a)
150.22 g Na2SO4
b)
593.44 g Na2SO4
c)
330.04 g Na2SO4
d)
297.65 g Na2SO4
97.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
98.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
99.

151 grams of Al2O3 are produced. How many grams of Al was needed in the reaction? Al + O2 -------> Al2O3 balance first.

a)

79.91 g

b)

22.4 liters

c)

57.8 g

d)

142.8 g

100.

What Mass of sulfur must burn to produce 3.42 L of SO2 @ 273K and 101 kPa?

Use the following Equation : S + O2 --> SO2

a)

2.45 g S

b)

5.00 g S

c)

4.88 g S

101.
If there are 5 boys and 7 girls, write the ratio of girls to boys.
a)
5 to 7
b)
7 to 5
c)
5 to 12
d)
7 to 12
102.

What is the ratio of red apples to green apples

a)

7 apples to 3 green

b)

4 red apples to 7 apples

c)

4 red apples to 3 green apples

d)

3 green apples to 4 red apples

103.

Mole Ratios used for conversions are derived from:

a)

the molar mass of the reactants in the balanced chemical equation

b)

the coefficients of the balanced chemical equation

c)

the subscripts of the products in the balanced chemical equation

d)

the group number of each element in the balanced chemical equation

104.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of ethane to oxygen gas?

a)
b)
c)
d)
105.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of carbon dioxide to water?

a)
b)
c)
d)
106.

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
107.
N2 +  3H2 → 2NH3 
What is the mole ratio between Nitrogen and Ammonium in the above reaction?
a)

1 moles NH3 / 2 moles N2 

b)

3 moles NH3 / 1 moles N2 

c)

2 moles N2 / 2 moles NH3 

d)

1 moles N2 / 2 moles NH3 

108.

2Na + S → Na2S

What is the ratio of Na2S to Na?

a)

1:1

b)

1:2

c)

2:1

d)

2:2

109.

4NH3 + 5O2 → 4NO + 6H2O

What is the mole ratio of water to oxygen?

a)

4/4

b)

4/5

c)

6/4

d)

6/5

110.

1 P4 + 3 O2 → 2 P2O3

What is the mole ratio of P4 to O2?

a)

1:3

b)

1:2

c)

3:2

d)

3:1

111.

3 CaCl2 + 2 Na3PO4 → Ca3(PO4)2 + 6 NaCl

What is the mole ratio of NaCl to Ca3(PO4)2?

a)

1:6

b)

6:1

c)

2:3

d)

3:2

112.

4 FeS + 7 O2 → 2 Fe2O3 + 4 SO2

What is the mole ratio of iron oxide to oxygen gas?

a)

4/7

b)

7/4

c)

2/7

d)

7/2

113.

4 FeS + 7 O2 → 2 Fe2O3 + 4 SO2

What is the mole ratio of iron sulfide to oxygen gas?

a)

4/7

b)

7/4

c)

2/7

d)

7/2

114.

3 Hg(OH)2 + 2 H3PO4 → Hg3(PO4)2 + 6 H2O

What is the mole ratio of Hg3(PO4)2 to H3PO4?

a)

1 to 2

b)

2 to 1

c)

2 to 3

d)

3 to 2

115.

3 Hg(OH)2 + 2 H3PO4 → Hg3(PO4)2 + 6 H2O

What is the mole ratio of Hg(OH)2 to Hg3(PO4)2 ?

a)

1 to 2

b)

2 to 1

c)

3 to 1

d)

1 to 3

116.

4 L = ____ mL

a)

40

b)

400

c)

4,000

d)

40,000

117.

5 kg = ______ g

a)

5

b)

50

c)

500

d)

5,000

118.

Which type of reaction is:

H2 + O2 → H2O

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

119.

Which type of reaction is:

NH3 + HCl → NH4Cl

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

120.

Which type of reaction is:

3Ca + 2AlCl3 --> 3CaCl2 + 2Al

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

121.

In which type of reaction does one element take the place of another element in a compound?

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

122.

In which type of reactions does one compound break down to form two or more simpler substances?

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

123.

In which type of reaction do two or more substances combine to form one new compound?

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

124.

In which type of reaction do the ions of two compounds switch places?

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

125.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

126.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

127.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
128.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
129.
Look at the diagram. In this diagram, the red dots represent
a)
the solute
b)
the solvent
c)
the solution
130.

Define the term soluble.

a)

Can dissolve in water

b)

Cannot dissolve in water

c)

Partially dissolves in water

131.

Define the term insoluble.

a)

Can dissolve in water.

b)

Cannot dissolve in water.

c)

Partially dissolves in water.

132.

Which factor affecting solubility is shown in the picture?

a)

temperature

b)

height

c)

stirring

d)

particle size

133.

Which factor is shown in the picture?

a)

temperature

b)

particle size

c)

stirring

d)

use of spoon

134.

Why do sugar particles dissolve faster in hot water?

a)

water particles move slow

b)

water particles move fast

c)

water particles settle down

d)

water particles stay on top

135.

How does particle size affect solubility?

a)

bigger particles dissolve faster

b)

smaller particles can occupy the space in water faster

c)

bigger particles spread faster than smaller particles

136.

What are the factors that affect solubility?

a)

rate of stirring

b)

particle size

c)

temperature

d)

all of these

137.

What combination would dissolve a solid solute the fastest?

a)

high temperature, no stirring

b)

no heat, no stirring

c)

sugar cube, no heat

d)

high temperature, stirring

138.
What is the formula for molarity?
a)
moles/grams
b)
moles/kilograms
c)
moles/milliliters
d)
moles/liters
139.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
140.
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
141.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
142.
When Koolaid mix is light colored and tastes watery it is a _______ solution.
a)
saturated 
b)
diluted
143.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
144.
When a certain amount of solvent cannot hold any more solute it is called a ________ solution.
a)
Diluted
b)
Saturated
145.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 

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