2nd Semester Exam online practice test

2nd Semester Exam PRACTICE

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Question 1

The compound shown is a(n):

A	carboxylic acid
B	amine
C	aldehyde
D	ester
E	ketone

Question 1 Explanation:

Organic Chemistry (Ch.25-26)

Question 2

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	180M
B	0.35M
C	2.8M
D	0.18M

Question 2 Explanation:

Solutions (Ch.18)

Question 3

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

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

Question 3 Explanation:

Water & Aqueous Systems (Ch.17)

Question 4

An ideal gas CANNOT be:

A	cooled
B	heated
C	liquefied
D	pressurized

Question 4 Explanation:

Gas Laws (Ch.12)

Question 5

Which of the following is NOT a phase change?

A	diffusion
B	melting
C	vaporization
D	sublimation

Question 5 Explanation:

States of Matter (Ch.10)

Question 6

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

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

Question 6 Explanation:

Acids & Bases (Ch. 20)

Question 7

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 kJ
C	0.2 kJ
D	2 J

Question 7 Explanation:

Thermochemistry (Ch.11)

Question 8

Why does a solute depress the freezing point?

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

Question 8 Explanation:

Solutions (Ch.18)

Question 9

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

Question 9 Explanation:

Solutions (Ch.18)

Question 10

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

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

Question 10 Explanation:

Acids & Bases (Ch. 20)

Question 11

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 combustion reaction
C	a combination reaction
D	exothermic

Question 11 Explanation:

Thermochemistry (Ch.11)

Question 12

What measuring instrument is used in a titration?

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

Question 12 Explanation:

Neutralization (Ch. 21)

Question 13

What type of reaction is an acid-base reaction?

A	double replacement
B	single replacement
C	decomposition
D	combination

Question 13 Explanation:

Neutralization (Ch. 21)

Question 14

Which structure below represents a ketone?

A
B
C
D
E

Question 14 Explanation:

Organic Chemistry (Ch.25-26)

Question 15

A solution is a mixture:

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

Question 15 Explanation:

Solutions (Ch.18)

Question 16

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

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

Question 16 Explanation:

Nuclear Chemistry (Ch.28)

Question 17

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

A	78
B	131
C	127
D	53

Question 17 Explanation:

Nuclear Chemistry (Ch.28)

Question 18

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

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

Question 18 Explanation:

Neutralization (Ch. 21)

Question 19

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

A	basic
B	it cannot be determined
C	neutral
D	acidic

Question 19 Explanation:

Acids & Bases (Ch. 20)

Question 20

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

Question 20 Explanation:

Thermochemistry (Ch.11)

Question 21

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

Question 21 Explanation:

Thermochemistry (Ch.11)

Question 22

What is the purpose of a titration?

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

Question 22 Explanation:

Neutralization (Ch. 20)

Question 23

Which of the following is a property of an acid?

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

Question 23 Explanation:

Acids & Bases (Ch. 20)

Question 24

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

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

Question 24 Explanation:

Gas Laws (Ch.12)

Question 25

The simplest alkyne is:

A	benzene
B	ethylene
C	ethane
D	acetylene
E	propyne

Question 25 Explanation:

Organic Chemistry (Ch.25-26)

Question 26

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

A	alpha particle
B	neutron
C	electron
D	proton

Question 26 Explanation:

Nuclear Chemistry (Ch.28)

Question 27

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

A	amides
B	aldehydes
C	esters
D	ketones
E	ethers

Question 27 Explanation:

Organic Chemistry (Ch.25-26)

Question 28

What type of reaction is known as a thermonuclear reaction?

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

Question 28 Explanation:

Nuclear Chemistry (Ch.28)

Question 29

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

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

Question 29 Explanation:

Gas Laws (Ch.12)

Question 30

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

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

Question 30 Explanation:

Solutions (Ch.18)

Question 31

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

Question 31 Explanation:

Solutions (Ch.18)

Question 32

Why does a higher concentration make a reaction faster?

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

Question 32 Explanation:

Solutions (Ch. 18)

Question 33

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 decreases.
C	The pressure does not change.

Question 33 Explanation:

Gas Laws (Ch.12)

Question 34

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

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

Question 34 Explanation:

Nuclear Chemistry (Ch.28)

Question 35

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

A	endothermic
B	exothermic
C	polythermic
D	ectothermic

Question 35 Explanation:

Thermochemistry (Ch.11)

Question 36

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

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

Question 36 Explanation:

Gas Laws (Ch.12)

Question 37

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	150 mL
D	67 mL
E	15 mL

Question 37 Explanation:

Solutions (Ch.18)

Question 38

Collisions between gas molecules are:

A	inelastic
B	never observed
C	elastic

Question 38 Explanation:

States of Matter (Ch.10)

Question 39

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

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

Question 39 Explanation:

Solutions (Ch.18)

Question 40

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

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

Question 40 Explanation:

Gas Laws (Ch.12)

Question 41

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 41 Explanation:

Solutions (Ch.18)

Question 42

What products result from a neutralization reaction?

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

Question 42 Explanation:

Neutralization (Ch. 21)

Question 43

Which atom in a water molecule has the greatest electronegativity?

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

Question 43 Explanation:

Water & Aqueous Systems (Ch.17)

Question 44

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

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

Question 44 Explanation:

Solutions (Ch.18)

Question 45

Hydrocarbons containing carbon-carbon triple bonds are called:

A	aromatic hydrocarbons
B	alkanes
C	alkenes
D	alkynes
E	olefins

Question 45 Explanation:

Organic Chemistry (Ch.25-26)

Question 46

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

Question 46 Explanation:

Organic Chemistry (Ch.25-26)

Question 47

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

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

Question 47 Explanation:

Water & Aqueous Systems (Ch.17)

Question 48

Alkynes always contain a:

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

Question 48 Explanation:

Organic Chemistry (Ch.25-26)

Question 49

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	420 cal
D	42,000 cal

Question 49 Explanation:

Thermochemistry (Ch.11)

Question 50

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	669 J
B	160 J
C	66.9 J
D	16.0 J

Question 50 Explanation:

Thermochemistry (Ch.11)

Question 51

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

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

Question 51 Explanation:

Thermochemistry (Ch.11)

Question 52

What does gamma radiation consist of?

A	hydrogen nuclei
B	helium nuclei
C	photons
D	electrons

Question 52 Explanation:

Nuclear Chemistry (Ch.28)

Question 53

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

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

Question 53 Explanation:

Acids & Bases (Ch. 20)

Question 54

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

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

Question 54 Explanation:

Solutions (Ch.18)

Question 55

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

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

Question 55 Explanation:

Solutions (Ch.18)

Question 56

Which type of ionizing radiation can be blocked by clothing?

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

Question 56 Explanation:

Nuclear Chemistry (Ch.28)

Question 57

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	1.25 mL
B	12.5 mL
C	5.0 mL
D	0.5 mL

Question 57 Explanation:

Solutions (Ch.18)

Question 58

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

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

Question 58 Explanation:

Solutions (Ch.18)

Question 59

What is a property of a base?

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

Question 59 Explanation:

Acids & Bases (Ch. 20)

Question 60

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

A	aromatics
B	alkenes
C	ketones
D	alkynes
E	alkanes

Question 60 Explanation:

Organic Chemistry (Ch.25-26)

Question 61

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

A	about the same
B	higher
C	lower

Question 61 Explanation:

Water & Aqueous Systems (Ch.17)

Question 62

What drives the turbine in a nuclear power plant?

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

Question 62 Explanation:

Nuclear Chemistry (Ch.28)

Question 63

What type of acid is sulfuric acid?

A	protic
B	diprotic
C	monoprotic
D	triprotic

Question 63 Explanation:

Acids & Bases (Ch. 20)

Question 64

When heat is added to boiling water, its temperature:

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

Question 64 Explanation:

Thermochemistry (Ch.11)

Question 65

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

A	8.6
B	8.3
C	8.0
D	9.3

Question 65 Explanation:

Acids & Bases (Ch. 20)

Question 66

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	30 g
C	7.5 g
D	3.0 g

Question 66 Explanation:

Solutions (Ch.18)

Question 67

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

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

Question 67 Explanation:

Gas Laws (Ch.12)

Question 68

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

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

Question 68 Explanation:

Nuclear Chemistry (Ch.28)

Question 69

The condensation of steam is a(n):

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

Question 69 Explanation:

Thermochemistry (Ch.11)

Question 70

What thickness of what material will stop gamma radiation?

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

Question 70 Explanation:

Nuclear Chemistry (Ch.28)

Question 71

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

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

Question 72

The bonds between adjacent water molecules are called:

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

Question 72 Explanation:

Water & Aqueous Systems (Ch.17)

Question 73

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 73 Explanation:

Nuclear Chemistry (Ch.28)

Question 74

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

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

Question 74 Explanation:

Nuclear Chemistry (Ch.28)

Question 75

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

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

Question 75 Explanation:

Nuclear Chemistry (Ch.28)

Question 76

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

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

Question 76 Explanation:

Solutions (Ch.18)

Question 77

What is the name of the compound shown?

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

Question 77 Explanation:

Organic Chemistry (Ch.25-26)

Question 78

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

Question 78 Explanation:

Gas Laws (Ch.12)

Question 79

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

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

Question 79 Explanation:

States of Matter (Ch.10)

Question 80

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

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

Question 80 Explanation:

Acids & Bases (Ch. 20)

Question 81

Standard conditions when working with gases are defined as:

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

Question 81 Explanation:

States of Matter (Ch.10)

Question 82

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

Question 82 Explanation:

Gas Laws (Ch.12)

Question 83

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

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

Question 83 Explanation:

Gas Laws (Ch.12)

Question 84

How many neutrons are there in an alpha particle?

A	2
B	0
C	1
D	4
E	3

Question 84 Explanation:

Nuclear Chemistry (Ch.28)

Question 85

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 increases
B	it decreases
C	it does not change

Question 85 Explanation:

Thermochemistry (Ch.11)

Question 86

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

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

Question 86 Explanation:

Thermochemistry (Ch.11)

Question 87

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

Question 87 Explanation:

Gas Laws (Ch.12)

Question 88

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

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

Question 88 Explanation:

Solutions (Ch.18)

Question 89

The structure of 2,3-dimethylheptane is:

A
B
C
D
E

Question 89 Explanation:

Organic Chemistry (Ch.25-26)

Question 90

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 90 Explanation:

Solutions (Ch.18)

Question 91

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

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

Question 91 Explanation:

Neutralization (Ch. 21)

Question 92

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

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

Question 92 Explanation:

Nuclear Chemistry (Ch.28)

Question 93

Most solids:

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

Question 93 Explanation:

States of Matter (Ch.10)

Question 94

The compound shown is an:

A	alkyne
B	olefin
C	alkane
D	alkene
E	aromatic compound

Question 94 Explanation:

Organic Chemistry (Ch.25-26)

Question 95

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	decreasing the temperature of a solution
C	increasing the temperature of a solution

Question 95 Explanation:

Solutions (Ch.18)

Question 96

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

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

Question 96 Explanation:

Solutions (Ch.18)

Question 97

What is the SI unit of pressure?

A	candela
B	mole
C	pascal
D	newton
E	joule

Question 97 Explanation:

States of Matter (Ch.10)

Question 98

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

A	-1.0
B	3.0
C	-3.0
D	11.0

Question 98 Explanation:

Acids & Bases (Ch. 20)

Question 99

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

Question 99 Explanation:

Gas Laws (Ch.12)

Question 100

Alkenes always contain a:

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

Question 100 Explanation:

Organic Chemistry (Ch.25-26)

Question 101

When gasoline is burned in an automobile engine:

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

Question 101 Explanation:

Thermochemistry (Ch.11)

Question 102

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

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

Question 102 Explanation:

Water & Aqueous Systems (Ch.17)

Question 103

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

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

Question 103 Explanation:

States of Matter (Ch.10)

Question 104

During a phase change, the temperature of a substance:

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

Question 104 Explanation:

Thermochemistry (Ch.11)

Question 105

What does the symbol "ΔH" stand for?

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

Question 105 Explanation:

Thermochemistry (Ch.11)

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