2nd Semester Exam online practice test

2nd Semester Exam PRACTICE

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Question 1

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

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

Question 1 Explanation:

Water & Aqueous Systems (Ch.17)

Question 2

The compound shown is a(n):

A	ester
B	aldehyde
C	carboxylic acid
D	ketone
E	amine

Question 2 Explanation:

Organic Chemistry (Ch.25-26)

Question 3

What measuring instrument is used in a titration?

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

Question 3 Explanation:

Neutralization (Ch. 21)

Question 4

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

Question 4 Explanation:

Solutions (Ch.18)

Question 5

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

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

Question 5 Explanation:

Solutions (Ch.18)

Question 6

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 does not change
B	it decreases
C	it increases

Question 6 Explanation:

Thermochemistry (Ch.11)

Question 7

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	endothermic
B	a combination reaction
C	a combustion reaction
D	exothermic

Question 7 Explanation:

Thermochemistry (Ch.11)

Question 8

What thickness of what material will stop gamma radiation?

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

Question 8 Explanation:

Nuclear Chemistry (Ch.28)

Question 9

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

A	alkanes
B	alkenes
C	aromatics
D	ketones
E	alkynes

Question 9 Explanation:

Organic Chemistry (Ch.25-26)

Question 10

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

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

Question 10 Explanation:

Nuclear Chemistry (Ch.28)

Question 11

Collisions between gas molecules are:

A	inelastic
B	elastic
C	never observed

Question 11 Explanation:

States of Matter (Ch.10)

Question 12

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

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

Question 12 Explanation:

Gas Laws (Ch.12)

Question 13

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

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

Question 13 Explanation:

Solutions (Ch.18)

Question 14

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

Question 14 Explanation:

Gas Laws (Ch.12)

Question 15

During a phase change, the temperature of a substance:

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

Question 15 Explanation:

Thermochemistry (Ch.11)

Question 16

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

A	basic
B	neutral
C	it cannot be determined
D	acidic

Question 16 Explanation:

Acids & Bases (Ch. 20)

Question 17

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

Question 17 Explanation:

Gas Laws (Ch.12)

Question 18

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

Question 18 Explanation:

Gas Laws (Ch.12)

Question 19

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

A	lower
B	higher
C	about the same

Question 19 Explanation:

Water & Aqueous Systems (Ch.17)

Question 20

What is the name of the compound shown?

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

Question 20 Explanation:

Organic Chemistry (Ch.25-26)

Question 21

Why does a higher concentration make a reaction faster?

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

Question 21 Explanation:

Solutions (Ch. 18)

Question 22

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

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

Question 22 Explanation:

Solutions (Ch.18)

Question 23

What is the purpose of a titration?

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

Question 23 Explanation:

Neutralization (Ch. 20)

Question 24

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

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

Question 24 Explanation:

Solutions (Ch.18)

Question 25

How many neutrons are there in an alpha particle?

A	4
B	2
C	0
D	3
E	1

Question 25 Explanation:

Nuclear Chemistry (Ch.28)

Question 26

The bonds between adjacent water molecules are called:

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

Question 26 Explanation:

Water & Aqueous Systems (Ch.17)

Question 27

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

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

Question 27 Explanation:

Solutions (Ch.18)

Question 28

What does gamma radiation consist of?

A	photons
B	hydrogen nuclei
C	helium nuclei
D	electrons

Question 28 Explanation:

Nuclear Chemistry (Ch.28)

Question 29

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

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

Question 29 Explanation:

Water & Aqueous Systems (Ch.17)

Question 30

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

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

Question 30 Explanation:

Neutralization (Ch. 21)

Question 31

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

A	because the pressure outside the tire is lower 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 greater than the pressure inside the tire
D	because the temperature is higher outside the tire than inside the tire

Question 31 Explanation:

Gas Laws (Ch.12)

Question 32

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	0.99 cal/g•°C
C	0.33 cal/g•°C
D	0.033 cal/g•°C

Question 32 Explanation:

Thermochemistry (Ch.11)

Question 33

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

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

Question 33 Explanation:

Solutions (Ch.18)

Question 34

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

A	11.0
B	-1.0
C	3.0
D	-3.0

Question 34 Explanation:

Acids & Bases (Ch. 20)

Question 35

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

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

Question 35 Explanation:

Solutions (Ch.18)

Question 36

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

Question 36 Explanation:

Thermochemistry (Ch.11)

Question 37

Which type of ionizing radiation can be blocked by clothing?

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

Question 37 Explanation:

Nuclear Chemistry (Ch.28)

Question 38

The structure of 2,3-dimethylheptane is:

A
B
C
D
E

Question 38 Explanation:

Organic Chemistry (Ch.25-26)

Question 39

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

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

Question 39 Explanation:

Solutions (Ch.18)

Question 40

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

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

Question 40 Explanation:

Solutions (Ch.18)

Question 41

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

A	aldehydes
B	ketones
C	esters
D	amides
E	ethers

Question 41 Explanation:

Organic Chemistry (Ch.25-26)

Question 42

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

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

Question 42 Explanation:

Gas Laws (Ch.12)

Question 43

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

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

Question 43 Explanation:

States of Matter (Ch.10)

Question 44

What is the SI unit of pressure?

A	candela
B	joule
C	pascal
D	mole
E	newton

Question 44 Explanation:

States of Matter (Ch.10)

Question 45

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

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

Question 45 Explanation:

Gas Laws (Ch.12)

Question 46

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	30 g
B	75 g
C	7.5 g
D	3.0 g

Question 46 Explanation:

Solutions (Ch.18)

Question 47

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

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

Question 47 Explanation:

Nuclear Chemistry (Ch.28)

Question 48

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

Question 48 Explanation:

Solutions (Ch.18)

Question 49

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

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

Question 49 Explanation:

Gas Laws (Ch.12)

Question 50

When gasoline is burned in an automobile engine:

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

Question 50 Explanation:

Thermochemistry (Ch.11)

Question 51

Alkenes always contain a:

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

Question 51 Explanation:

Organic Chemistry (Ch.25-26)

Question 52

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

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

Question 52 Explanation:

Nuclear Chemistry (Ch.28)

Question 53

What type of acid is sulfuric acid?

A	protic
B	triprotic
C	diprotic
D	monoprotic

Question 53 Explanation:

Acids & Bases (Ch. 20)

Question 54

Which of the following is a property of an acid?

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

Question 54 Explanation:

Acids & Bases (Ch. 20)

Question 55

Why does a solute depress the freezing point?

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

Question 55 Explanation:

Solutions (Ch.18)

Question 56

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	12.5 mL
B	5.0 mL
C	1.25 mL
D	0.5 mL

Question 56 Explanation:

Solutions (Ch.18)

Question 57

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

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

Question 57 Explanation:

Thermochemistry (Ch.11)

Question 58

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

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

Question 58 Explanation:

Acids & Bases (Ch. 20)

Question 59

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

A	53
B	127
C	78
D	131

Question 59 Explanation:

Nuclear Chemistry (Ch.28)

Question 60

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

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

Question 60 Explanation:

Neutralization (Ch. 21)

Question 61

What drives the turbine in a nuclear power plant?

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

Question 61 Explanation:

Nuclear Chemistry (Ch.28)

Question 62

Which atom in a water molecule has the greatest electronegativity?

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

Question 62 Explanation:

Water & Aqueous Systems (Ch.17)

Question 63

An ideal gas CANNOT be:

A	liquefied
B	heated
C	pressurized
D	cooled

Question 63 Explanation:

Gas Laws (Ch.12)

Question 64

Most solids:

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

Question 64 Explanation:

States of Matter (Ch.10)

Question 65

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

A	electron
B	proton
C	neutron
D	alpha particle

Question 65 Explanation:

Nuclear Chemistry (Ch.28)

Question 66

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

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

Question 66 Explanation:

Acids & Bases (Ch. 20)

Question 67

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

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

Question 67 Explanation:

Water & Aqueous Systems (Ch.17)

Question 68

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

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

Question 68 Explanation:

Acids & Bases (Ch. 20)

Question 69

What products result from a neutralization reaction?

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

Question 69 Explanation:

Neutralization (Ch. 21)

Question 70

Hydrocarbons containing carbon-carbon triple bonds are called:

A	alkanes
B	alkenes
C	olefins
D	alkynes
E	aromatic hydrocarbons

Question 70 Explanation:

Organic Chemistry (Ch.25-26)

Question 71

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

A	8.0
B	8.6
C	8.3
D	9.3

Question 71 Explanation:

Acids & Bases (Ch. 20)

Question 72

A solution is a mixture:

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

Question 72 Explanation:

Solutions (Ch.18)

Question 73

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 73 Explanation:

Thermochemistry (Ch.11)

Question 74

The compound shown is an:

A	alkene
B	olefin
C	aromatic compound
D	alkyne
E	alkane

Question 74 Explanation:

Organic Chemistry (Ch.25-26)

Question 75

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

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

Question 75 Explanation:

Solutions (Ch.18)

Question 76

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

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

Question 76 Explanation:

Nuclear Chemistry (Ch.28)

Question 77

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	0.18M
B	2.8M
C	180M
D	0.35M

Question 77 Explanation:

Solutions (Ch.18)

Question 78

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

Question 78 Explanation:

Solutions (Ch.18)

Question 79

What is a property of a base?

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

Question 79 Explanation:

Acids & Bases (Ch. 20)

Question 80

Which of the following is NOT a phase change?

A	vaporization
B	melting
C	diffusion
D	sublimation

Question 80 Explanation:

States of Matter (Ch.10)

Question 81

When heat is added to boiling water, its temperature:

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

Question 81 Explanation:

Thermochemistry (Ch.11)

Question 82

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

Question 82 Explanation:

Organic Chemistry (Ch.25-26)

Question 83

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

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

Question 83 Explanation:

Nuclear Chemistry (Ch.28)

Question 84

The simplest alkyne is:

A	propyne
B	ethane
C	acetylene
D	benzene
E	ethylene

Question 84 Explanation:

Organic Chemistry (Ch.25-26)

Question 85

What type of reaction is known as a thermonuclear reaction?

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

Question 85 Explanation:

Nuclear Chemistry (Ch.28)

Question 86

Standard conditions when working with gases are defined as:

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

Question 86 Explanation:

States of Matter (Ch.10)

Question 87

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

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

Question 87 Explanation:

Gas Laws (Ch.12)

Question 88

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	669 J
C	66.9 J
D	160 J

Question 88 Explanation:

Thermochemistry (Ch.11)

Question 89

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

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

Question 89 Explanation:

Solutions (Ch.18)

Question 90

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

A	ectothermic
B	exothermic
C	polythermic
D	endothermic

Question 90 Explanation:

Thermochemistry (Ch.11)

Question 91

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

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

Question 91 Explanation:

States of Matter (Ch.10)

Question 92

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

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

Question 92 Explanation:

Nuclear Chemistry (Ch.28)

Question 93

If an isotope undergoes beta emission:

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

Question 93 Explanation:

Nuclear Chemistry (Ch.28)

Question 94

Alkynes always contain a:

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

Question 94 Explanation:

Organic Chemistry (Ch.25-26)

Question 95

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

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

Question 95 Explanation:

Thermochemistry (Ch.11)

Question 96

What does the symbol "ΔH" stand for?

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

Question 96 Explanation:

Thermochemistry (Ch.11)

Question 97

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

Question 97 Explanation:

Thermochemistry (Ch.11)

Question 98

Which structure below represents a ketone?

A
B
C
D
E

Question 98 Explanation:

Organic Chemistry (Ch.25-26)

Question 99

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

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

Question 99 Explanation:

Acids & Bases (Ch. 20)

Question 100

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

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

Question 101

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

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

Question 101 Explanation:

Gas Laws (Ch.12)

Question 102

What type of reaction is an acid-base reaction?

A	decomposition
B	single replacement
C	combination
D	double replacement

Question 102 Explanation:

Neutralization (Ch. 21)

Question 103

The condensation of steam is a(n):

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

Question 103 Explanation:

Thermochemistry (Ch.11)

Question 104

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

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

Question 104 Explanation:

Solutions (Ch.18)

Question 105

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 105 Explanation:

Gas Laws (Ch.12)

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