2nd Semester Exam online practice test

2nd Semester Exam PRACTICE

Please wait while the activity loads.
If this activity does not load, try refreshing your browser. Also, this page requires javascript. Please visit using a browser with javascript enabled.

If loading fails, click here to try again

For each of the following questions, please select the MOST correct answer by clicking on its letter:

Start

Congratulations - you have completed 2nd Semester Exam PRACTICE. You scored %%SCORE%% out of %%TOTAL%%. Your performance has been rated as %%RATING%%

Your answers are highlighted below.

Question 1

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

A	alpha particle
B	proton
C	electron
D	neutron

Question 1 Explanation:

Nuclear Chemistry (Ch.28)

Question 2

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

A	acidic
B	basic
C	neutral
D	it cannot be determined

Question 2 Explanation:

Acids & Bases (Ch. 20)

Question 3

Most solids:

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

Question 3 Explanation:

States of Matter (Ch.10)

Question 4

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 4 Explanation:

Thermochemistry (Ch.11)

Question 5

What type of reaction is known as a thermonuclear reaction?

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

Question 5 Explanation:

Nuclear Chemistry (Ch.28)

Question 6

What drives the turbine in a nuclear power plant?

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

Question 6 Explanation:

Nuclear Chemistry (Ch.28)

Question 7

The condensation of steam is a(n):

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

Question 7 Explanation:

Thermochemistry (Ch.11)

Question 8

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

Question 8 Explanation:

Gas Laws (Ch.12)

Question 9

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

A	endothermic
B	ectothermic
C	polythermic
D	exothermic

Question 9 Explanation:

Thermochemistry (Ch.11)

Question 10

Which type of ionizing radiation can be blocked by clothing?

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

Question 10 Explanation:

Nuclear Chemistry (Ch.28)

Question 11

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

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

Question 11 Explanation:

Acids & Bases (Ch. 20)

Question 12

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

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

Question 12 Explanation:

Solutions (Ch.18)

Question 13

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 13 Explanation:

Water & Aqueous Systems (Ch.17)

Question 14

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	0.18M
C	180M
D	0.35M

Question 14 Explanation:

Solutions (Ch.18)

Question 15

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

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

Question 15 Explanation:

Gas Laws (Ch.12)

Question 16

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 16 Explanation:

Gas Laws (Ch.12)

Question 17

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

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

Question 17 Explanation:

Nuclear Chemistry (Ch.28)

Question 18

What is a property of a base?

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

Question 18 Explanation:

Acids & Bases (Ch. 20)

Question 19

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

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

Question 19 Explanation:

Water & Aqueous Systems (Ch.17)

Question 20

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

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

Question 20 Explanation:

Solutions (Ch.18)

Question 21

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	higher
D	cannot be determined

Question 21 Explanation:

Water & Aqueous Systems (Ch.17)

Question 22

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

Question 22 Explanation:

Organic Chemistry (Ch.25-26)

Question 23

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 23 Explanation:

Solutions (Ch.18)

Question 24

How many neutrons are there in an alpha particle?

A	4
B	3
C	1
D	0
E	2

Question 24 Explanation:

Nuclear Chemistry (Ch.28)

Question 25

Which of the following is a property of an acid?

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

Question 25 Explanation:

Acids & Bases (Ch. 20)

Question 26

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

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

Question 26 Explanation:

Nuclear Chemistry (Ch.28)

Question 27

What measuring instrument is used in a titration?

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

Question 27 Explanation:

Neutralization (Ch. 21)

Question 28

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

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

Question 28 Explanation:

Nuclear Chemistry (Ch.28)

Question 29

When gasoline is burned in an automobile engine:

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

Question 29 Explanation:

Thermochemistry (Ch.11)

Question 30

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

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

Question 30 Explanation:

Gas Laws (Ch.12)

Question 31

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

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

Question 31 Explanation:

Gas Laws (Ch.12)

Question 32

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

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

Question 32 Explanation:

Solutions (Ch.18)

Question 33

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	0.83M
C	0.24M
D	2.4M
E	0.30M

Question 33 Explanation:

Solutions (Ch.18)

Question 34

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

A	8.3
B	8.0
C	9.3
D	8.6

Question 34 Explanation:

Acids & Bases (Ch. 20)

Question 35

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

A	78
B	53
C	131
D	127

Question 35 Explanation:

Nuclear Chemistry (Ch.28)

Question 36

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

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

Question 36 Explanation:

Solutions (Ch.18)

Question 37

The structure of 2,3-dimethylheptane is:

A
B
C
D
E

Question 37 Explanation:

Organic Chemistry (Ch.25-26)

Question 38

Alkenes always contain a:

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

Question 38 Explanation:

Organic Chemistry (Ch.25-26)

Question 39

What does the symbol "ΔH" stand for?

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

Question 39 Explanation:

Thermochemistry (Ch.11)

Question 40

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

A	ethers
B	amides
C	esters
D	aldehydes
E	ketones

Question 40 Explanation:

Organic Chemistry (Ch.25-26)

Question 41

Which of the following is NOT a phase change?

A	diffusion
B	vaporization
C	sublimation
D	melting

Question 41 Explanation:

States of Matter (Ch.10)

Question 42

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	2 kJ
D	0.2 kJ

Question 42 Explanation:

Thermochemistry (Ch.11)

Question 43

An ideal gas CANNOT be:

A	heated
B	cooled
C	pressurized
D	liquefied

Question 43 Explanation:

Gas Laws (Ch.12)

Question 44

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 44 Explanation:

Solutions (Ch. 18)

Question 45

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

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

Question 45 Explanation:

Nuclear Chemistry (Ch.28)

Question 46

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	66.9 J
C	160 J
D	669 J

Question 46 Explanation:

Thermochemistry (Ch.11)

Question 47

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

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

Question 47 Explanation:

Water & Aqueous Systems (Ch.17)

Question 48

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	7.5 g
B	3.0 g
C	30 g
D	75 g

Question 48 Explanation:

Solutions (Ch.18)

Question 49

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

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

Question 49 Explanation:

Nuclear Chemistry (Ch.28)

Question 50

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

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

Question 50 Explanation:

Solutions (Ch.18)

Question 51

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

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

Question 51 Explanation:

Solutions (Ch.18)

Question 52

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

Question 52 Explanation:

Gas Laws (Ch.12)

Question 53

Alkynes always contain a:

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

Question 53 Explanation:

Organic Chemistry (Ch.25-26)

Question 54

During a phase change, the temperature of a substance:

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

Question 54 Explanation:

Thermochemistry (Ch.11)

Question 55

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

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

Question 55 Explanation:

Neutralization (Ch. 21)

Question 56

What is the purpose of a titration?

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

Question 56 Explanation:

Neutralization (Ch. 20)

Question 57

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

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

Question 57 Explanation:

Acids & Bases (Ch. 20)

Question 58

What is the name of the compound shown?

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

Question 58 Explanation:

Organic Chemistry (Ch.25-26)

Question 59

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	0.5 mL
B	12.5 mL
C	5.0 mL
D	1.25 mL

Question 59 Explanation:

Solutions (Ch.18)

Question 60

When heat is added to boiling water, its temperature:

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

Question 60 Explanation:

Thermochemistry (Ch.11)

Question 61

Collisions between gas molecules are:

A	never observed
B	inelastic
C	elastic

Question 61 Explanation:

States of Matter (Ch.10)

Question 62

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

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

Question 62 Explanation:

Solutions (Ch.18)

Question 63

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 63 Explanation:

Solutions (Ch.18)

Question 64

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	4200 cal
D	420 cal

Question 64 Explanation:

Thermochemistry (Ch.11)

Question 65

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

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

Question 65 Explanation:

Solutions (Ch.18)

Question 66

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

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

Question 66 Explanation:

Solutions (Ch.18)

Question 67

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

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

Question 67 Explanation:

States of Matter (Ch.10)

Question 68

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⁺ + H₂O
C	MgH₂ + H₃SO₄
D	MgSO₄ + H₃O⁺ + OH^-

Question 68 Explanation:

Neutralization (Ch. 21)

Question 69

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

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

Question 69 Explanation:

Solutions (Ch.18)

Question 70

What type of reaction is an acid-base reaction?

A	double replacement
B	single replacement
C	combination
D	decomposition

Question 70 Explanation:

Neutralization (Ch. 21)

Question 71

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 increase in the force of the collisions between the particles and the walls of the container
C	because there is a corresponding decrease in volume
D	because there is a corresponding increase in the temperature

Question 71 Explanation:

Gas Laws (Ch.12)

Question 72

The simplest alkyne is:

A	ethylene
B	acetylene
C	propyne
D	ethane
E	benzene

Question 72 Explanation:

Organic Chemistry (Ch.25-26)

Question 73

What products result from a neutralization reaction?

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

Question 73 Explanation:

Neutralization (Ch. 21)

Question 74

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 metal will increase.
C	The temperature of the water 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 74 Explanation:

Thermochemistry (Ch.11)

Question 75

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 75 Explanation:

Water & Aqueous Systems (Ch.17)

Question 76

Hydrocarbons containing carbon-carbon triple bonds are called:

A	alkanes
B	alkynes
C	aromatic hydrocarbons
D	olefins
E	alkenes

Question 76 Explanation:

Organic Chemistry (Ch.25-26)

Question 77

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	I only
D	II only
E	II and III

Question 77 Explanation:

Solutions (Ch.18)

Question 78

Which structure below represents a ketone?

A
B
C
D
E

Question 78 Explanation:

Organic Chemistry (Ch.25-26)

Question 79

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

A	3.0
B	-3.0
C	-1.0
D	11.0

Question 79 Explanation:

Acids & Bases (Ch. 20)

Question 80

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 80 Explanation:

Gas Laws (Ch.12)

Question 81

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

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

Question 81 Explanation:

Thermochemistry (Ch.11)

Question 82

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

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

Question 82 Explanation:

States of Matter (Ch.10)

Question 83

What thickness of what material will stop gamma radiation?

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

Question 83 Explanation:

Nuclear Chemistry (Ch.28)

Question 84

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

Question 84 Explanation:

Solutions (Ch.18)

Question 85

What is the SI unit of pressure?

A	mole
B	newton
C	joule
D	pascal
E	candela

Question 85 Explanation:

States of Matter (Ch.10)

Question 86

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 combustion reaction
B	a combination reaction
C	exothermic
D	endothermic

Question 86 Explanation:

Thermochemistry (Ch.11)

Question 87

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 disrupts crystal formation by the solvent
C	because the solute is colder than the solvent
D	because the solute has bigger molecules than the solvent

Question 87 Explanation:

Solutions (Ch.18)

Question 88

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 88 Explanation:

Thermochemistry (Ch.11)

Question 89

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

A	alkanes
B	alkenes
C	aromatics
D	alkynes
E	ketones

Question 89 Explanation:

Organic Chemistry (Ch.25-26)

Question 90

If an isotope undergoes beta emission:

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

Question 90 Explanation:

Nuclear Chemistry (Ch.28)

Question 91

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	Additional amounts of the same gas are added to the container.
D	The temperature is increased.

Question 91 Explanation:

Gas Laws (Ch.12)

Question 92

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

Question 92 Explanation:

Gas Laws (Ch.12)

Question 93

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

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

Question 93 Explanation:

Acids & Bases (Ch. 20)

Question 94

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

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

Question 94 Explanation:

Gas Laws (Ch.12)

Question 95

The compound shown is an:

A	olefin
B	alkane
C	alkyne
D	alkene
E	aromatic compound

Question 95 Explanation:

Organic Chemistry (Ch.25-26)

Question 96

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

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

Question 96 Explanation:

Acids & Bases (Ch. 20)

Question 97

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

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

Question 97 Explanation:

Solutions (Ch.18)

Question 98

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

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

Question 98 Explanation:

Nuclear Chemistry (Ch.28)

Question 99

Standard conditions when working with gases are defined as:

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

Question 99 Explanation:

States of Matter (Ch.10)

Question 100

The bonds between adjacent water molecules are called:

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

Question 100 Explanation:

Water & Aqueous Systems (Ch.17)

Question 101

What does gamma radiation consist of?

A	hydrogen nuclei
B	electrons
C	photons
D	helium nuclei

Question 101 Explanation:

Nuclear Chemistry (Ch.28)

Question 102

What type of acid is sulfuric acid?

A	monoprotic
B	triprotic
C	diprotic
D	protic

Question 102 Explanation:

Acids & Bases (Ch. 20)

Question 103

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

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

Question 104

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 104 Explanation:

Thermochemistry (Ch.11)

Question 105

The compound shown is a(n):

A	aldehyde
B	ketone
C	carboxylic acid
D	amine
E	ester

Question 105 Explanation:

Organic Chemistry (Ch.25-26)

Once you are finished, click the button below. Any items you have not completed will be marked incorrect. Get Results

There are 105 questions to complete.

←

List

→

Return

Shaded items are complete.

1	2	3	4	5
6	7	8	9	10
11	12	13	14	15
16	17	18	19	20
21	22	23	24	25
26	27	28	29	30
31	32	33	34	35
36	37	38	39	40
41	42	43	44	45
46	47	48	49	50
51	52	53	54	55
56	57	58	59	60
61	62	63	64	65
66	67	68	69	70
71	72	73	74	75
76	77	78	79	80
81	82	83	84	85
86	87	88	89	90
91	92	93	94	95
96	97	98	99	100
101	102	103	104	105
End

Return

Mr. Carman's Blog

2nd Semester Exam online practice test

2nd Semester Exam PRACTICE

Assignments, resources, links and more!