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Final Exam Units 3, 4, 4.1, and 4.2 iTeachly 24-25

Total questions: 126

Worksheet time: 4hrs 1mins

Name
Class
Date
1.

Which of the following is generally an irreversible process?

a)

Chemical change

b)

Physical change

c)

Freezing

d)

Boiling

2.

In which of the following reactions, is a new substance formed?

a)

Sugar crystals are dissolved in hot water.

b)

Boiling of water and formation of steam.

c)

Cutting of an apple into two pieces.

d)

Burning of wood and formation of ash and fumes.

3.

Which of the following is a chemical change?

a)

Boiling of water

b)

Tearing of paper

c)

Formation of ice

d)

Rusting of iron

4.

_____________________ are ingredients of a chemical reaction.

a)

Reactants

b)

Products

c)

Reagents

d)

Enzymes

5.

A + B → C + D. In the given reaction, what are C and D?

a)

Reactants

b)

Products

c)

Reagents

d)

Enzymes

6.

Which of the following is/are chemical changes during a chemical reaction?

a)

Change in color

b)

Formation of precipitate

c)

Release of heat and light

d)

All the above

7.

Which process produces a chemical change?

a)

Physical reaction

b)

Chemical reaction

c)

Any reaction

d)

Evaporation

8.

Burning of something is called ________________________.

a)

solidification

b)

combustion

c)

evaporation

d)

condensation

9.

Which of the following is an example of an exothermic reaction?

a)

Freezing of water into ice

b)

Melting of water

c)

Photosynthesis

d)

Combustion

10.

If more energy is produced during a chemical reaction than utilized in the reaction, it is a/an _____________________ reaction.

a)

endothermic

b)

exothermic

c)

endergonic

d)

evaporation

11.

A campfire is an example of

a)

Exothermic reaction

b)

Endothermic reaction

c)

Physical change

d)

Sublimation

12.

Which of the following is an endothermic reaction?

a)

Rusting of iron

b)

Combustion of fuel

c)

Sugar burning

d)

Photosynthesis

13.

Which of the following equations does not observe the law of conservation of mass?

a)

b)

c)

d)

14.

18.02g of water are separated by electrolysis into hydrogen and oxygen gas. If 16.00g of oxygen gas are obtained, how much hydrogen gas is obtained?

a)

16.00g

b)

1.01g

c)

8.00g

d)

2.02g

15.

Iron reacts with oxygen to form ferrous oxide, commonly known as rust. If 55.85g of iron completely reacts with 24.00g oxygen. What is the mass of the rust formed?

a)

79.85g

b)

55.85g

c)

24.00g

d)

111.70g

16.

The composition of pure substances can be described as...

a)

Equal

b)

Definite

c)

Constant

d)

Absolute

17.

How do elements combine?

a)

In whole numbers

b)

By halves

c)

Randomly

d)

In portions

18.

Find the mass ratio of ammonia (NH3)

a)

3:1

b)

1:3

c)

3:14

d)

14:3

19.

Which of the following is an example of a synthesis reaction?

a)

C + O2 --> CO2

b)

MgCO3 --> MgO + CO2

c)

2AgNO3 + Ni --> Ni(NO3)2 + 2Ag

d)

H2SO4 --> H2O + SO3

20.

Which of the following is an example of a decomposition reaction?

a)

b)

c)

d)

21.

Use the reactivity series to help you determine which of the following is more reactive.

Which the most reactive metal in each case.

a)

Calcium

b)

Potassium

22.

What reaction has the following general formula:
CxHy + O2 −>CO2 + H2OC_xH_y\ +\ O_2\ ->CO_{2\ }+\ H_2O  

a)

Combination

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

23.

What type of reaction is the following:
3CuS +2Al −> Al2S3+3Cu3CuS\ +2Al\ ->\ Al_2S_3+3Cu

a)

Combination

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

24.
2 NaBr + 1 Ca(OH)2 ----> 1 CaBr2 + 2 NaOH
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
25.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)

Fe + 3 O2 → Fe2O3

b)

3 Fe + 3 O2 → 2 Fe2O3

c)

2 Fe + O2 → Fe2O3

d)

4 Fe + 3 O2 → 2 Fe2O3

26.
If an element is diatomic it should have a subscript of___
a)
2, always
b)
2, only when it is by itself
c)
it shouldn't have a subscript, it should have a coefficent
27.
What is the product when rubidium and oxygen gas react?
a)
RbO2
b)
Rb2O
c)
RbO
d)
Rb2O2
28.

Predict the products of the following decomposition reaction, before balancing.

HgO -->

a)

Hg + O

b)

Hg2 + O2

c)

Hg + O2

d)

Hg2 + O

29.

What is the charge of Iron in this compound. (Hint: think swap drop method):

Fe3(PO4)2

a)

3+

b)

2+

c)

1+

d)

6+

30.

Predict the products, before balancing.

Co2(SO4)3 + NaOH -->

a)

CoOH + NaSO4

b)

CoNa + OH(SO4)3

c)

Co2OH + Na(SO4)3

d)

Co(OH)3 + Na2SO4

e)

no reaction

31.

What are the products for this combustion reaction:

C2H4 + 2 O2 -->

a)

C2O2 + H4

b)

CO2 + HOH

c)

CO + H

d)

CO2 + H2O

32.

The symbol for a substance dissolved in solution is ______

a)

(s)

b)

(l)

c)

(aq)

d)

(g)

33.

A type of chemical that forms solutions that taste sour, due to high concentrations of positive hydrogen ions

a)

acid

b)

base

c)

salt

d)

pH

34.

What is considered to be in the middle of the pH scale

a)

acidic

b)

neutral

c)

basic

d)

indicator

35.
If there is excess hydroxide ions, the solution will be...
a)
acidic
b)
basic
36.
Identify the salt in the following equation:
Zn(OH)2 + HNO3   ---> H2O  + Zn(NO3)2
a)
Zn(OH)2
b)
HNO3
c)
H2O
d)
Zn(NO3)2
37.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

38.

What coefficeient is needed to balance the equation?

N2 + _H2 -> 2NH3

a)

2

b)

6

c)

1

d)

3

39.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
40.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
41.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products 
c)
Yields 
d)
Chemical Equation 
42.
Balance this equation-
__P4 + __O2 --> __P2O3
a)
it is already balanced
b)
2, 1, 3
c)
1, 2, 3
d)
1, 3, 2
43.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
44.

What is the arrow in a chemical equation...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

45.
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
46.
What is oxidation number of Mn in MnO2?
a)
0
b)
+2
c)
-2
d)
+4
47.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
48.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
49.

Is combining sand an example of a chemical or physical change?

a)

Chemical

b)

Physical

50.

Atomic mass is the...

a)

Number of neutrons found in an atom

b)

The number of protons found in an atom

c)

The number of protons and neutrons found in an atom

d)

The number of protons, neutrons and electrons found in an atom

51.

The atomic mass of carbon is...

a)

6

b)

12

c)

18

d)

24

52.

The molar mass of carbon is...

a)

The same as the atomic mass

b)

The same as the atomic number

c)

The atomic number plus the mass number

d)

The mass number minus the atomic number

53.

The unit for molar mass is...

a)

moles

b)

grams

c)

grams per mole

d)

moles per liter

54.

One mole contains _____________ atoms/particles.

a)

6.02 x1020

b)

6.02 x1021

c)

6.02 x1022

d)

6.02 x1023

55.

What is the molar mass of Ca(OH)2, rounded to the nearest whole number?

a)

114 g

b)

40 g

c)

57 g

d)

74 g

56.

How many molecules are in 2.5 mol of NaCl?

a)

1.51x1023

b)

146

c)

4.15

d)

1.51x1024

57.

How many moles are equal to 89.23 g of calcium oxide, CaO? (Molar Mass = 56.1 g/mol)

a)

1.59 mol

b)

2.03 mol

c)

1.77 mol

d)

3.21 mol

58.

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

59.

How many molecules of water are in a 821.3 g sample? (Molar Mass = 18 g/mol)

a)

45.58 molecules

b)

8.232 x 1025 molecules

c)

8.909 x 1027 molecules

d)

2.744 x 1025 molecules

60.

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

61.

Find the percent composition of hydrogen in (NH4)2S. (Molar Mass = 68.1 g/mol)

a)
11.8%
b)
41.1%
c)
47.1%
62.

The molar mass of water is ____ g/mol.

a)

2

b)

14

c)

16

d)

18

63.

What percentage by mass of carbon in the compound carbon dioxide (CO2)?

(Molar Mass = 44 g/mol)

a)

12%

b)

27%

c)

73%

d)

44%

64.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

65.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

66.

What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 60.053 g/mol?

a)

C3H6O3

b)

C2H4O2

c)

C4H8O4

d)

C6H12O6

e)

C5H10O5

67.

A hydrocarbon is 85.7% carbon and 14.3% hydrogen with an empirical formula of CH2.

If its molar mass is 84 g/mol which of the following is the compounds molecular formula?

a)

C4H8

b)

C6H12

c)

C6H16

d)

C10H20

68.
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
69.
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
70.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
71.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
72.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
73.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
74.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
75.
Which is NOT an assumption made by the kinetic molecular theory of gases?
a)
Gas particles are small and take up little volume
b)
Particles travel in constant, random, straight-line motion until colliding
c)
When particles collide, their total kinetic energy is decreased
d)
Particles do not attract or repel each other
e)

The temperature of a gas depends on the average kinetic energy of the gas particles.

76.

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?

Hint: Use Boyle's Law

a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
77.

What is -50oC in Kelvin?

a)
223
b)
323
c)
100
d)
50
78.

4. According to Charles Law, the relationship between Temperature and Volume can best be described as....

a)

Inversely proportional

b)

Directly proportional

c)

No Relationship

79.

If the temperature of a gas increases, the pressure...

Gay-Lussac's Law

a)

Decreases

b)

Increases

c)

Does not change

80.

A quantity of gas has a volume of 250 L, at 290 K and 2280 Torr of pressure. What volume must the gas be for the gas to be at 32oF and 760 Torr?

Hint: Use the Combined gas law

a)

78.4 L

b)

88.5 L

c)

706 L

d)

771 L

81.
Molar volume of any gas at STP
a)
22.4 L
b)
2.24 L
c)
6.02 x 1023 L
d)
224 L
82.

A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?

Hint: Use Molar Volume

a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
83.

When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pressure of 700 mm Hg. What is the volume of the container?

Hint: Ideal Gas Law

a)
0.557 Liters
b)
6.57 Liters
c)
8.74 Liters
d)
0.0087 Liters
84.

Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

Hint: Use Molar volume

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

85.

Container T is made combining all the gases from containers A, B, and C. What is the pressure in container C?

Hint: Use Dalton's Law

a)

200kPa

b)

550kPa

c)

250kPa

d)

150kPa

86.

A gaseous mixture contains 5.0 moles of nitrogen and 10.0 moles of helium. The total pressure in the container is 3.0 atmospheres. What is the partial pressure of the nitrogen?

a)

1 atm

b)

0.5 atm

c)

3.0 atm

d)

2.0 atm

87.

why would O2 effuse faster than CO2 in the same room

a)

because O2 has more energy

b)

because CO2 has a greater molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

88.

how many times faster does He effuse compared to N2 (Molar Masses: He = 4  N2 = 28)

Hint: Use Graham's Law

a)
1.2 times faster
b)
2.65 times faster
c)
7 times faster
d)
0.377 times faster
89.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
90.
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
91.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

92.

What mass of water should be added to 22.0 g of KCl to make 5.50% by mass solution?

a)

400 g

b)

40 g

c)

0.25 g

d)

25 g

93.

If 25.0 mL of ethanol is dissolved in enough water to make 500 mL of solution, what is the percent by volume of ethanol in the solution?

a)

5.0%

b)

0.5%

c)

2.5%

94.

Calculate the molality if you have 0.1 moles of solute and 300 grams of solvent.

a)

0.9 mol/L

b)

0.01 m

c)

0.33 m

d)

30 mol/kg

95.

What is the molality of a solution which contains 30.0 g of CaCl2 dissolved in 150 g of H2O

a)

2.6 m

b)

1.8 m

c)

0.2 m

d)

0.05 m

96.

Determine the freezing point of a 0.08 m solution dissolved in water (0°C freezing point and Kf = 1.86°C)

a)

-0.15 °C

b)

0.004 °C

c)

1 °C

d)

-11 °C

97.

Nitrates (NO3-)

a)

Soluble

b)

Insoluble

98.

Carbonates and Chromates

a)

Soluble

b)

Insoluble

99.
Silver Iodide
a)
Soluble 
b)
Insoluble 
100.
KOH
a)
Soluble 
b)
Insoluble
101.
Ca(OH)2
a)
soluble
b)
insoluble
102.

Using the supplied solubility curve diagram, determine the temperature at which KNO3 and NH4Cl have the same solubility.

a)

16°C

b)

39°C

c)

25°C

d)

73°C

103.

Using the supplied solubility curve diagram, determine what type of solution would be present if 50 grams of NH3 was dissolved in 100 grams of water at 30°C.

a)

saturated

b)

unsaturated

c)

supersaturated

104.

Using the supplied solubility curve diagram, determine which compound listed below is least soluble at 70°C.

a)

NH4Cl

b)

NaCl

c)

KCl

d)

KNO3

105.

What are the spectator ions in the reaction of sodium chloride with silver nitrate?

Na+(aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) --> Na+(aq) + AgCl (s) + NO3- (aq)

a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
106.
Which of these results in formation of a precipitate?
a)
BaNO3(aq)  +  NaCl(aq)→
b)
KNO3(aq)  +  LiOH(aq)→
c)
Zn(NO3)2(aq)  +  NaOH(aq)→
d)
NaNO3(aq)  +  Ba(OH)2(aq)→
107.

HCl is:

a)

an Arrhenius acid

b)

a Bronsted Lowry acid

c)

both an Arrhenius and Bronsted Lowry acid

d)

a base

108.

NaOH is:

a)

an Arrhenius base

b)

an Arrhenius acid

c)

neither an acid nor a base

d)

both an acid and a base

109.

An Arrhenius base:

a)

donates H+

b)

accepts H+

c)

produces H+

d)

produces OH-

110.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

111.

NH3 + H2O --> NH4+ + OH-

What is NH4+ in this reaction?

a)

acid

b)

base

c)

conjugate acid

d)

conjugate base

112.

In the equation below, what is the conjugate base?

HBr + H2O ↔ Br- + H3O+

a)

HBr

b)

H2O

c)

Br-

d)

H3O+

113.

Given the reaction above, which compound is the acid?

a)

NH3

b)

HCl

c)

NH4+

d)

Cl-

114.

What is the name of the following acid or base?
HNO3

a)

Nitric acid

b)

Hydronitric acid

c)

Nitrous acid

115.

What is the name of the following acid or base?
HCl

a)

hydrochloric acid

b)

chloric acid

c)

chlorous acid

116.

What is the name of the following acid or base?
H2SO4

a)

sulfuric acid

b)

hydrosulfuric acid

c)

sulfurous acid

117.

What is the name of the following acid or base?
HNO2

a)

nitrous acid

b)

hydronitric acid

c)

nitric acid

118.

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

119.

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

a)

Acid

b)

Base

c)

Neutral

120.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
121.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
122.

The pH of a solution is 8.43. What is the hydronium ion H3O+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

123.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
124.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

125.

What is the endpoint of a titration

a)

Where the amount of acid and base are equal as shown by a color change

b)

Where there is no base

c)

When the volume of base in the burette is used up

d)

When there is no acid

126.
The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H2O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if the is 15.0mL of acid neutralized?
a)
0.8M
b)
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