2nd Semester Exam online practice test

2nd Semester Exam PRACTICE

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Question 1

Which structure below represents a ketone?

A
B
C
D
E

Question 1 Explanation:

Organic Chemistry (Ch.25-26)

Question 2

An ideal gas CANNOT be:

A	liquefied
B	heated
C	cooled
D	pressurized

Question 2 Explanation:

Gas Laws (Ch.12)

Question 3

How many mL of 3M HCl are needed to make 300 mL of 0.1M HCl?

A	90 mL
B	9 mL
C	100 mL
D	30 mL
E	10 mL

Question 3 Explanation:

Solutions (Ch.18)

Question 4

When an acid reacts with a base what compounds are formed?

A	metal oxides only
B	a salt only
C	a salt and water
D	water only

Question 4 Explanation:

Acids & Bases (Ch. 20)

Question 5

A process that absorbs heat is a(n) ________process.

A	endothermic
B	exothermic
C	ectothermic
D	polythermic

Question 5 Explanation:

Thermochemistry (Ch.11)

Question 6

If the hydrogen ion concentration in a solution is is 10^-10 M, is it acidic, basic, or neutral?

A	acidic
B	basic
C	it cannot be determined
D	neutral

Question 6 Explanation:

Acids & Bases (Ch. 20)

Question 7

What is the volume of alcohol present in 200.0 mL of a 55% (v/v) solution of alcohol?

A	36 mL
B	28 mL
C	145 mL
D	110 mL

Question 7 Explanation:

Solutions (Ch.18)

Question 8

Alkynes always contain a:

A	C=H bond
B	C=C bond
C	C-C bond
D	C≡C bond
E	C≡H bond

Question 8 Explanation:

Organic Chemistry (Ch.25-26)

Question 9

A sample of gas occupies 40.0 mL at -123°C. What volume does the sample occupy at 27°C?

A	20.0 mL
B	182 mL
C	8.80 mL
D	80.0 mL

Question 9 Explanation:

Gas Laws (Ch.12)

Question 10

What is the change in atomic number when an atom emits gamma radiation?

A	decreases by 1
B	remains the same
C	increases by 1
D	increases by 2
E	decreases by 2

Question 10 Explanation:

Nuclear Chemistry (Ch.28)

Question 11

Why does air leave a tire when the tire valve is opened?

A	because the pressure outside the tire is greater than the pressure inside the tire
B	because there are more gas particles outside the tire than inside the tire
C	because the pressure outside the tire is lower than the pressure inside the tire
D	because the temperature is higher outside the tire than inside the tire

Question 11 Explanation:

Gas Laws (Ch.12)

Question 12

Which of the following is NOT a colligative property of a solution?

A	boiling point elevation
B	freezing point depression
C	vapor pressure lowering
D	supersaturation

Question 12 Explanation:

Solutions (Ch.18)

Question 13

If more solvent is added to a solution, which of the following does NOT happen?

A	it becomes more dilute
B	its vapor pressure decreases
C	its percent (v/v) decreases
D	its molarity decreases

Question 13 Explanation:

Solutions (Ch.18)

Question 14

As the temperature of a sample of matter is increased, what happens to the average kinetic energy of the particles in the sample?

A	it decreases
B	it does not change
C	it increases

Question 14 Explanation:

Thermochemistry (Ch.11)

Question 15

What is the pH of a solution with [H⁺] = 4.5 x 10^-9?

A	8.0
B	9.3
C	8.3
D	8.6

Question 15 Explanation:

Acids & Bases (Ch. 20)

Question 16

What does the symbol "ΔH" stand for?

A	one Calorie given off by a reaction
B	the heat of reaction for a chemical reaction
C	the specific heat of a substance
D	the heat capacity of a substance

Question 16 Explanation:

Thermochemistry (Ch.11)

Question 17

If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in solution?

A	5.0 mL
B	0.5 mL
C	1.25 mL
D	12.5 mL

Question 17 Explanation:

Solutions (Ch.18)

Question 18

What is the molarity of a solution containing 9.0 moles of solute in 500.0 mL of solution?

A	18 M
B	0.18 M
C	4.5 M
D	0.45 M
E	1.8 M

Question 18 Explanation:

Solutions (Ch.18)

Question 19

How many neutrons are in the nucleus of iodine-131 (atomic number 53)?

A	131
B	78
C	127
D	53

Question 19 Explanation:

Nuclear Chemistry (Ch.28)

Question 20

What is the purpose of a titration?

A	to determine the concentration of acid or base
B	to determine the volume of base
C	to determine the concentration of acid only
D	to determine the color of an indicator

Question 20 Explanation:

Neutralization (Ch. 20)

Question 21

What is the change in the atomic number when an atom emits an alpha particle?

A	decreases by 1
B	increases by 2
C	remains the same
D	decreases by 2
E	increases by 1

Question 21 Explanation:

Nuclear Chemistry (Ch.28)

Question 22

The structure of 2,3-dimethylheptane is:

A
B
C
D
E

Question 22 Explanation:

Organic Chemistry (Ch.25-26)

Question 23

How does the surface tension of water compare with the surface tensions of most other liquids?

A	about the same
B	lower
C	higher

Question 23 Explanation:

Water & Aqueous Systems (Ch.17)

Question 24

When gasoline is burned in an automobile engine:

A	energy is destroyed
B	heat energy is converted to chemical energy
C	energy is created
D	potential energy is transformed into kinetic energy

Question 24 Explanation:

Thermochemistry (Ch.11)

Question 25

What is the volume occupied by 2.20 mol of hydrogen at STP?

A	2.60 L
B	24.6 L
C	2.20 L
D	49.3 L
E	98.6 L

Question 25 Explanation:

States of Matter (Ch.10)

Question 26

Alcohols are hydrocarbon derivatives in which one or more hydrogens have been replaced by a hydroxyl functional group. What is the general formula of an alcohol?

A	R-CO-OH
B	R-CO-R
C	R-OH
D	R-O-R
E	R-CO-H

Question 26 Explanation:

Organic Chemistry (Ch.25-26)

Question 27

When heat is added to boiling water, its temperature:

A	depends on the amount of water
B	increases
C	decreases
D	stays the same

Question 27 Explanation:

Thermochemistry (Ch.11)

Question 28

Standard conditions when working with gases are defined as:

A	0 K and 101 kPa
B	0°C and 10 kPa
C	0 K and 10 kPa
D	0°C and 101 kPa

Question 28 Explanation:

States of Matter (Ch.10)

Question 29

What happens to the pressure of a gas inside a container if the temperature of the gas is lowered?

A	The pressure increases.
B	The pressure does not change.
C	The pressure decreases.

Question 29 Explanation:

Gas Laws (Ch.12)

Question 30

Why does a solute depress the freezing point?

A	because the solute tends to sink to the bottom of the solution
B	because the solute is colder than the solvent
C	because the solute has bigger molecules than the solvent
D	because the solute disrupts crystal formation by the solvent

Question 30 Explanation:

Solutions (Ch.18)

Question 31

Which type of ionizing radiation can be blocked by clothing?

A	alpha particle
B	beta particle
C	X-radiation
D	gamma radiation

Question 31 Explanation:

Nuclear Chemistry (Ch.28)

Question 32

Which of the following is primarily responsible for holding water molecules together in the liquid state?

A	polar covalent bonds
B	dispersion forces
C	hydrogen bonds
D	ionic bonds

Question 32 Explanation:

Water & Aqueous Systems (Ch.17)

Question 33

If a stock solution of hydrochloric acid is 3.0M, how many milliliters are needed to make 200.0 mL of 0.10M HCl?

A	150 mL
B	1.5 mL
C	15 mL
D	6.7 mL
E	67 mL

Question 33 Explanation:

Solutions (Ch.18)

Question 34

The volume of a gas is reduced from 4 L to 0.5 L while the temperature is held constant. How does the gas pressure change?

A	increases by a factor of two
B	increases by a factor of eight
C	decreases by a factor of eight
D	increases by a factor of four

Question 34 Explanation:

Gas Laws (Ch.12)

Question 35

The compound shown is a(n):

A	amine
B	ester
C	ketone
D	aldehyde
E	carboxylic acid

Question 35 Explanation:

Organic Chemistry (Ch.25-26)

Question 36

How many neutrons are there in an alpha particle?

A	4
B	2
C	1
D	0
E	3

Question 36 Explanation:

Nuclear Chemistry (Ch.28)

Question 37

Which of the following is NOT a phase change?

A	melting
B	diffusion
C	vaporization
D	sublimation

Question 37 Explanation:

States of Matter (Ch.10)

Question 38

What is the molarity of a solution containing 8 grams of solute in 500 mL of solution? (molar mass of solute = 24 g)

A	1 M
B	0.05 M
C	0.1 M
D	0.5 M
E	0.67 M

Question 38 Explanation:

Solutions (Ch.18)

Question 39

To what does plutonium-239 (atomic number 94) decay when it loses an alpha particle?

A	uranium-235
B	thorium-237
C	plutonium-235
D	americium-239

Question 39 Explanation:

Nuclear Chemistry (Ch.28)

Question 40

What is the volume occupied by 71 g of chlorine gas at STP?

A	44.8 L
B	22.4 L
C	56.0 L
D	67.2 L
E	78.4 L

Question 40 Explanation:

States of Matter (Ch.10)

Question 41

What mass of Na₂SO₄ is needed to make 2.5 L of 2.0M solution?

A	178 g
B	284 g
C	356 g
D	710 g

Question 41 Explanation:

Solutions (Ch.18)

Question 42

Hydrocarbons containing only single bonds between the carbon atoms are called:

A	aromatics
B	alkynes
C	ketones
D	alkanes
E	alkenes

Question 42 Explanation:

Organic Chemistry (Ch.25-26)

Question 43

What is the number of grams of neon present in 78.4 L of neon at STP?

A	140 g
B	105 g
C	35 g
D	20 g
E	70 g

Question 44

What does not change when a solution is diluted by the addition of solvent?

A	number of moles of solute
B	mass of solution
C	molarity of solution
D	volume of solvent
E	mass of solvent

Question 44 Explanation:

Solutions (Ch.18)

Question 45

Increasing the rate at which a solute dissolves and the amount of solute that dissolves can be accomplished by:

A	increasing the temperature of a solution
B	keeping the temperature of a solution constant
C	decreasing the temperature of a solution

Question 45 Explanation:

Solutions (Ch.18)

Question 46

A solution is a mixture:

A	from which the solute can be filtered
B	that is heterogeneous
C	that has the same properties throughout
D	in which a solid solute is always dissolved in a liquid solvent

Question 46 Explanation:

Solutions (Ch.18)

Question 47

What are the products of the reaction of one mole of Mg(OH)₂ and one mole of H₂SO₄?

A	MgH₂ + H₃SO₄
B	MgSO₄ + H₃O⁺ + OH^-
C	MgSO₄ + 2 H₂O
D	MgSO₄ + H₃O⁺ + H₂O

Question 47 Explanation:

Neutralization (Ch. 21)

Question 48

When 1.0 g of solid NaOH (ΔHsoln = -44.51 kJ/mol) dissolves in 10 L of water, how much heat is released?

A	1.11 kJ
B	44.51 kJ
C	1.11 J
D	40.51 kJ

Question 48 Explanation:

Thermochemistry (Ch.11)

Question 49

What is the name of the compound shown?

A	2,4-methylbutene
B	2,4-ethylbutene
C	2,5-dimethylpentane
D	2,4-dimethyl-1-pentene
E	2,4-dimethyl-4-pentene

Question 49 Explanation:

Organic Chemistry (Ch.25-26)

Question 50

Holding the temperature constant while adding more solute to a solution that already has solute crystals at the bottom of the container:

A	makes the solution more concentrated
B	causes the solution to become supersaturated
C	causes more solute crystals to appear at the bottom of the container

Question 50 Explanation:

Solutions (Ch.18)

Question 51

If an isotope undergoes beta emission:

A	the number of neutrons remains the same
B	protons are given off
C	the atomic number changes
D	the mass number changes

Question 51 Explanation:

Nuclear Chemistry (Ch.28)

Question 52

What does the ideal gas law allow a scientist to calculate that the other laws do not?

A	temperature
B	energy
C	number of moles
D	pressure
E	volume

Question 52 Explanation:

Gas Laws (Ch.12)

Question 53

What measuring instrument is used in a titration?

A	volumetric pipette
B	Erlenmeyer flask
C	syringe
D	graduated cylinder
E	buret

Question 53 Explanation:

Neutralization (Ch. 21)

Question 54

What does gamma radiation consist of?

A	helium nuclei
B	electrons
C	hydrogen nuclei
D	photons

Question 54 Explanation:

Nuclear Chemistry (Ch.28)

Question 55

At a certain temperature and pressure, 0.20 mol of CO₂ has a volume of 3.1 L. A 3.1-L sample of hydrogen at the same temperature and pressure:

A	contains the same number of atoms
B	contains the same number of molecules
C	has a higher density
D	has the same mass

Question 55 Explanation:

Gas Laws (Ch.12)

Question 56

If the pH of a solution is 6, what is its concentration of hydrogen ions?

A	10^-6 M
B	10^-7 M
C	10^-8 M
D	10^-14 M
E	10^-1 M

Question 56 Explanation:

Acids & Bases (Ch. 20)

Question 57

What particle does argon-39 (atomic number 18) lose when it decays to potassium-39 (atomic number 19)?

A	proton
B	alpha particle
C	electron
D	neutron

Question 57 Explanation:

Nuclear Chemistry (Ch.28)

Question 58

During a phase change, the temperature of a substance:

A	remains constant
B	decreases
C	increases
D	may increase or decrease

Question 58 Explanation:

Thermochemistry (Ch.11)

Question 59

What thickness of what material will stop gamma radiation?

A	one inch of water
B	sheet of paper
C	sheet of aluminum foil
D	three inches of lead

Question 59 Explanation:

Nuclear Chemistry (Ch.28)

Question 60

Which of the following operations usually makes a substance dissolve faster in a solvent? I. crushing the substance to a powder II. raising the temperature III. agitation

A	I and II
B	II only
C	II and III
D	I only
E	I, II and III

Question 60 Explanation:

Solutions (Ch.18)

Question 61

When cooking food with natural gas, the energy comes from:

A	the volume of the gas
B	kinetic energy in the gas
C	the pressure of the gas
D	chemical potential energy of the gas molecules

Question 61 Explanation:

Thermochemistry (Ch.11)

Question 62

What type of reaction is known as a thermonuclear reaction?

A	neutron emission
B	fission
C	transmutation
D	beta emission
E	fusion

Question 62 Explanation:

Nuclear Chemistry (Ch.28)

Question 63

What is the SI unit of pressure?

A	pascal
B	joule
C	mole
D	newton
E	candela

Question 63 Explanation:

States of Matter (Ch.10)

Question 64

What mass of sucrose, C₁₂H₂₂O₁₁, is needed to make 500.0 mL of a 0.200M solution?

A	34.2 g
B	17.1 g
C	68.4 g
D	100 g

Question 64 Explanation:

Solutions (Ch.18)

Question 65

Why does a higher temperature cause a reaction to go faster?

A	There are more collisions per second only.
B	Collisions occur with greater energy only.
C	There are more collisions per second and the collisions are of greater energy.

Question 65 Explanation:

Solutions (Ch.18)

Question 66

What is the concentration of hydronium ions in a neutral solution?

A	No determination can be made from the information given
B	10^-7 M
C	10⁰ M
D	10^-10 M

Question 66 Explanation:

Acids & Bases (Ch. 20)

Question 67

The simplest alkyne is:

A	acetylene
B	ethane
C	ethylene
D	benzene
E	propyne

Question 67 Explanation:

Organic Chemistry (Ch.25-26)

Question 68

Most solids:

A	are dense and incompressible
B	consist of particles in chaotic motion
C	are amorphous in nature
D	have high melting points

Question 68 Explanation:

States of Matter (Ch.10)

Question 69

If [H⁺] = 1 x 10^-11 M, what is the pH of the solution?

A	-3.0
B	3.0
C	11.0
D	-1.0

Question 69 Explanation:

Acids & Bases (Ch. 20)

Question 70

Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base?

A	hydrochloric acid
B	sodium chloride
C	sodium hydroxide
D	ammonia
E	water

Question 70 Explanation:

Acids & Bases (Ch. 20)

Question 71

Which of the following compounds does not contain a C=O bond?

A	esters
B	aldehydes
C	amides
D	ethers
E	ketones

Question 71 Explanation:

Organic Chemistry (Ch.25-26)

Question 72

If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change within the container?

A	The pressure will be four times as great.
B	The pressure will be twice as great.
C	The pressure will not change.
D	The pressure will be five times as great.

Question 72 Explanation:

Gas Laws (Ch.12)

Question 73

The compound shown is an:

A	alkane
B	alkyne
C	olefin
D	alkene
E	aromatic compound

Question 73 Explanation:

Organic Chemistry (Ch.25-26)

Question 74

If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?

A	0.024M
B	2.4M
C	0.30M
D	0.24M
E	0.83M

Question 74 Explanation:

Solutions (Ch.18)

Question 75

When 10 g of diethyl ether is converted to vapor at its boiling point, about how much heat is absorbed? (C₄H₁₀O, ΔH_vap = 15.7 kJ/mol, boiling point: 34.6°C)

A	2 J
B	Not enough information given
C	0.2 kJ
D	2 kJ

Question 75 Explanation:

Thermochemistry (Ch.11)

Question 76

The bonds between adjacent water molecules are called:

A	nonpolar covalent bonds
B	polar covalent bonds
C	hydrogen bonds
D	ionic bonds

Question 76 Explanation:

Water & Aqueous Systems (Ch.17)

Question 77

What is the specific heat of a substance if 1560 cal is required to raise the temperature of a 312 g sample by 15°C?

A	1.33 cal/g•°C
B	0.033 cal/g•°C
C	0.99 cal/g•°C
D	0.33 cal/g•°C

Question 77 Explanation:

Thermochemistry (Ch.11)

Question 78

Why does a higher concentration make a reaction faster?

A	Collisions occur with greater energy.
B	There are more collisions per second and the collisions are of greater energy.
C	There are more collisions per second only.

Question 78 Explanation:

Solutions (Ch. 18)

Question 79

Hydrocarbons containing carbon-carbon triple bonds are called:

A	alkenes
B	olefins
C	alkynes
D	aromatic hydrocarbons
E	alkanes

Question 79 Explanation:

Organic Chemistry (Ch.25-26)

Question 80

Which of the following is a property of an acid?

A	sour taste
B	nonelectrolyte
C	slippery feel
D	unreactive
E	strong color

Question 80 Explanation:

Acids & Bases (Ch. 20)

Question 81

What type of reaction is an acid-base reaction?

A	decomposition
B	single replacement
C	combination
D	double replacement

Question 81 Explanation:

Neutralization (Ch. 21)

Question 82

A gas occupies a volume of 0.7 L at 10.1 kPa. What volume will the gas occupy at 101 kPa?

A	0.7 L
B	0.07 L
C	4 L
D	7 L

Question 82 Explanation:

Gas Laws (Ch.12)

Question 83

What type of acid is sulfuric acid?

A	diprotic
B	triprotic
C	monoprotic
D	protic

Question 83 Explanation:

Acids & Bases (Ch. 20)

Question 84

Which of the following is NOT one of the assumptions of kinetic theory?

A	Gases consist of hard spherical particles.
B	All gas particles move in constant random motion.
C	Particles in a gas are assumed to have an insignificant volume.
D	Only small attractive and repulsive forces exists between gas particles.

Question 84 Explanation:

Gas Laws (Ch.12)

Question 85

A student adds enough water to 225-mL of a 0.80M solution of KI to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?

A	2.8M
B	0.35M
C	180M
D	0.18M

Question 85 Explanation:

Solutions (Ch.18)

Question 86

Which of these changes would NOT cause an increase in the pressure of a gaseous system?

A	The temperature is increased.
B	Additional amounts of the same gas are added to the container.
C	Another gas is added to the container.
D	The container is made larger.

Question 86 Explanation:

Gas Laws (Ch.12)

Question 87

What thickness of what material is necessary to stop a beta particle?

A	sheet of aluminum foil
B	three feet of concrete
C	sheet of paper
D	three inches of lead

Question 87 Explanation:

Nuclear Chemistry (Ch.28)

Question 88

What thickness of what material is necessary to stop an alpha particle?

A	sheet of aluminum foil
B	sheet of paper
C	three feet of concrete
D	three inches of lead

Question 88 Explanation:

Nuclear Chemistry (Ch.28)

Question 89

What is a property of a base?

A	watery feel
B	strong color
C	unreactive
D	nonelectrolyte
E	bitter taste

Question 89 Explanation:

Acids & Bases (Ch. 20)

Question 90

Alkenes always contain a:

A	C≡C bond
B	C=H bond
C	C≡H bond
D	C-C bond
E	C=C bond

Question 90 Explanation:

Organic Chemistry (Ch.25-26)

Question 91

How much heat does it take to warm 16.0 g of pure water from 90.0°C to 100.0°C? (specific heat of water = 4.18 J/(g•°C) )

A	16.0 J
B	160 J
C	66.9 J
D	669 J

Question 91 Explanation:

Thermochemistry (Ch.11)

Question 92

What is obtained when phosphoric acid and magnesium hydroxide are mixed?

A	hydrogen gas
B	hydrogen-magnesium alloy
C	water only
D	magnesium hydride
E	magnesium phosphate plus water

Question 92 Explanation:

Neutralization (Ch. 21)

Question 93

Why does the pressure inside a container of gas increase if more gas is added to the container?

A	because there is a corresponding increase in the number of particles striking an area of the wall of the container per unit time
B	because there is a corresponding decrease in volume
C	because there is a corresponding increase in the temperature
D	because there is a corresponding increase in the force of the collisions between the particles and the walls of the container

Question 93 Explanation:

Gas Laws (Ch.12)

Question 94

What drives the turbine in a nuclear power plant?

A	the primary coolant
B	UF₆ gas
C	the control rods
D	steam
E	the moderator

Question 94 Explanation:

Nuclear Chemistry (Ch.28)

Question 95

If the percent (mass/volume) for the solute is 4% and the volume of the solution is 750 mL, what is the mass of solute in solution?

A	75 g
B	3.0 g
C	7.5 g
D	30 g

Question 95 Explanation:

Solutions (Ch.18)

Question 96

Collisions between gas molecules are:

A	never observed
B	inelastic
C	elastic

Question 96 Explanation:

States of Matter (Ch.10)

Question 97

What is the change in atomic number when an atom emits a beta particle?

A	+2
B	+1
C	-2
D	0
E	-1

Question 97 Explanation:

Nuclear Chemistry (Ch.28)

Question 98

The bonds between the hydrogen and oxygen atoms in a water molecule are:

A	hydrogen bonds
B	nonpolar covalent bonds
C	ionic bonds
D	polar covalent bonds

Question 98 Explanation:

Water & Aqueous Systems (Ch.17)

Question 99

How does the boiling point of water compare with the boiling points of other molecules of similar size?

A	cannot be determined
B	about the same
C	lower
D	higher

Question 99 Explanation:

Water & Aqueous Systems (Ch.17)

Question 100

A piece of metal is heated, then submerged in cool water. Which statement below describes what happens?

A	The temperature of the water will increase and the temperature of the metal will decrease.
B	The temperature of the metal will increase.
C	The temperature of the water will decrease and the temperature of the metal will increase.
D	The temperature of the water will decrease.
E	The temperature of the water will increase.

Question 100 Explanation:

Thermochemistry (Ch.11)

Question 101

What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (specific heat of aluminum = 0.21 cal/(g•°C) )

A	4200 cal
B	420,000 cal
C	42,000 cal
D	420 cal

Question 101 Explanation:

Thermochemistry (Ch.11)

Question 102

Which atom in a water molecule has the greatest electronegativity?

A	both hydrogen atoms
B	one of the hydrogen atoms
C	there is no difference in the electronegativities of the atoms in a water molecule
D	the oxygen atom

Question 102 Explanation:

Water & Aqueous Systems (Ch.17)

Question 103

The following equation shows the reaction that occurs when nitroglycerine explodes.

4 C₃H₅O₉N₃ → 12 CO₂ + 6 N₂ + O₂ + 10 H₂O + 1725 kcal This reaction is:

A	a combination reaction
B	endothermic
C	a combustion reaction
D	exothermic

Question 103 Explanation:

Thermochemistry (Ch.11)

Question 104

What products result from a neutralization reaction?

A	water only
B	a salt only
C	a salt and water
D	acids and bases
E	polar covalent compounds

Question 104 Explanation:

Neutralization (Ch. 21)

Question 105

The condensation of steam is a(n):

A	catalytic process
B	endothermic process
C	exothermic process
D	electrolytic process

Question 105 Explanation:

Thermochemistry (Ch.11)

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