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

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 1 Explanation:

Solutions (Ch.18)

Question 2

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

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

Question 2 Explanation:

Gas Laws (Ch.12)

Question 3

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

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

Question 3 Explanation:

Water & Aqueous Systems (Ch.17)

Question 4

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

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

Question 4 Explanation:

Solutions (Ch.18)

Question 5

What products result from a neutralization reaction?

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

Question 5 Explanation:

Neutralization (Ch. 21)

Question 6

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

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

Question 6 Explanation:

States of Matter (Ch.10)

Question 7

What is the SI unit of pressure?

A	joule
B	candela
C	pascal
D	newton
E	mole

Question 7 Explanation:

States of Matter (Ch.10)

Question 8

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

A	alkenes
B	alkynes
C	alkanes
D	ketones
E	aromatics

Question 8 Explanation:

Organic Chemistry (Ch.25-26)

Question 9

The compound shown is an:

A	alkyne
B	aromatic compound
C	alkene
D	alkane
E	olefin

Question 9 Explanation:

Organic Chemistry (Ch.25-26)

Question 10

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

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

Question 10 Explanation:

States of Matter (Ch.10)

Question 11

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

Question 11 Explanation:

Thermochemistry (Ch.11)

Question 12

Why does a solute depress the freezing point?

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

Question 12 Explanation:

Solutions (Ch.18)

Question 13

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

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

Question 13 Explanation:

Nuclear Chemistry (Ch.28)

Question 14

Alkynes always contain a:

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

Question 14 Explanation:

Organic Chemistry (Ch.25-26)

Question 15

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

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

Question 15 Explanation:

Solutions (Ch.18)

Question 16

What type of reaction is known as a thermonuclear reaction?

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

Question 16 Explanation:

Nuclear Chemistry (Ch.28)

Question 17

Alkenes always contain a:

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

Question 17 Explanation:

Organic Chemistry (Ch.25-26)

Question 18

Hydrocarbons containing carbon-carbon triple bonds are called:

A	olefins
B	alkenes
C	aromatic hydrocarbons
D	alkanes
E	alkynes

Question 18 Explanation:

Organic Chemistry (Ch.25-26)

Question 19

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 cal
C	42,000 cal
D	420,000 cal

Question 19 Explanation:

Thermochemistry (Ch.11)

Question 20

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

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

Question 20 Explanation:

Neutralization (Ch. 21)

Question 21

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

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

Question 21 Explanation:

Gas Laws (Ch.12)

Question 22

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

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

Question 22 Explanation:

Acids & Bases (Ch. 20)

Question 23

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

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

Question 23 Explanation:

Nuclear Chemistry (Ch.28)

Question 24

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

Question 24 Explanation:

Solutions (Ch.18)

Question 25

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

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

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

Question 26 Explanation:

Organic Chemistry (Ch.25-26)

Question 27

What thickness of what material will stop gamma radiation?

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

Question 27 Explanation:

Nuclear Chemistry (Ch.28)

Question 28

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	0.2 kJ
C	2 kJ
D	Not enough information given

Question 28 Explanation:

Thermochemistry (Ch.11)

Question 29

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

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

Question 29 Explanation:

Water & Aqueous Systems (Ch.17)

Question 30

Which of the following is NOT a phase change?

A	melting
B	sublimation
C	diffusion
D	vaporization

Question 30 Explanation:

States of Matter (Ch.10)

Question 31

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

Question 31 Explanation:

Solutions (Ch.18)

Question 32

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 32 Explanation:

Solutions (Ch.18)

Question 33

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

Question 33 Explanation:

Gas Laws (Ch.12)

Question 34

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

A	3.0
B	-1.0
C	-3.0
D	11.0

Question 34 Explanation:

Acids & Bases (Ch. 20)

Question 35

Standard conditions when working with gases are defined as:

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

Question 35 Explanation:

States of Matter (Ch.10)

Question 36

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	makes the solution more concentrated
C	causes more solute crystals to appear at the bottom of the container

Question 36 Explanation:

Solutions (Ch.18)

Question 37

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 37 Explanation:

Solutions (Ch. 18)

Question 38

What is the purpose of a titration?

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

Question 38 Explanation:

Neutralization (Ch. 20)

Question 39

What type of reaction is an acid-base reaction?

A	double replacement
B	single replacement
C	combination
D	decomposition

Question 39 Explanation:

Neutralization (Ch. 21)

Question 40

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

A	higher
B	lower
C	about the same

Question 40 Explanation:

Water & Aqueous Systems (Ch.17)

Question 41

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

A	ectothermic
B	exothermic
C	polythermic
D	endothermic

Question 41 Explanation:

Thermochemistry (Ch.11)

Question 42

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⁺ + H₂O
C	MgSO₄ + H₃O⁺ + OH^-
D	MgSO₄ + 2 H₂O

Question 42 Explanation:

Neutralization (Ch. 21)

Question 43

When gasoline is burned in an automobile engine:

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

Question 43 Explanation:

Thermochemistry (Ch.11)

Question 44

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

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

Question 44 Explanation:

Thermochemistry (Ch.11)

Question 45

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

Question 45 Explanation:

Gas Laws (Ch.12)

Question 46

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	2.8M
C	0.18M
D	0.35M

Question 46 Explanation:

Solutions (Ch.18)

Question 47

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

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

Question 47 Explanation:

Water & Aqueous Systems (Ch.17)

Question 48

An ideal gas CANNOT be:

A	pressurized
B	liquefied
C	cooled
D	heated

Question 48 Explanation:

Gas Laws (Ch.12)

Question 49

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 49 Explanation:

Thermochemistry (Ch.11)

Question 50

What drives the turbine in a nuclear power plant?

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

Question 50 Explanation:

Nuclear Chemistry (Ch.28)

Question 51

What does gamma radiation consist of?

A	electrons
B	photons
C	helium nuclei
D	hydrogen nuclei

Question 51 Explanation:

Nuclear Chemistry (Ch.28)

Question 52

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

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

Question 52 Explanation:

Nuclear Chemistry (Ch.28)

Question 53

What measuring instrument is used in a titration?

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

Question 53 Explanation:

Neutralization (Ch. 21)

Question 54

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

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

Question 54 Explanation:

Acids & Bases (Ch. 20)

Question 55

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 decreases.
C	The pressure increases.

Question 55 Explanation:

Gas Laws (Ch.12)

Question 56

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

Question 56 Explanation:

Gas Laws (Ch.12)

Question 57

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	0.1 M
C	0.5 M
D	1 M
E	0.67 M

Question 57 Explanation:

Solutions (Ch.18)

Question 58

What is a property of a base?

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

Question 58 Explanation:

Acids & Bases (Ch. 20)

Question 59

The simplest alkyne is:

A	acetylene
B	ethane
C	propyne
D	benzene
E	ethylene

Question 59 Explanation:

Organic Chemistry (Ch.25-26)

Question 60

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 60 Explanation:

Nuclear Chemistry (Ch.28)

Question 61

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

A	8.6
B	8.0
C	9.3
D	8.3

Question 61 Explanation:

Acids & Bases (Ch. 20)

Question 62

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

A	esters
B	amides
C	ethers
D	aldehydes
E	ketones

Question 62 Explanation:

Organic Chemistry (Ch.25-26)

Question 63

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 63 Explanation:

Solutions (Ch.18)

Question 64

During a phase change, the temperature of a substance:

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

Question 64 Explanation:

Thermochemistry (Ch.11)

Question 65

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

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

Question 65 Explanation:

Solutions (Ch.18)

Question 66

Collisions between gas molecules are:

A	elastic
B	inelastic
C	never observed

Question 66 Explanation:

States of Matter (Ch.10)

Question 67

Which type of ionizing radiation can be blocked by clothing?

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

Question 67 Explanation:

Nuclear Chemistry (Ch.28)

Question 68

Most solids:

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

Question 68 Explanation:

States of Matter (Ch.10)

Question 69

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 69 Explanation:

Solutions (Ch.18)

Question 70

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 70 Explanation:

Thermochemistry (Ch.11)

Question 71

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 71 Explanation:

Solutions (Ch.18)

Question 72

The compound shown is a(n):

A	aldehyde
B	ketone
C	ester
D	amine
E	carboxylic acid

Question 72 Explanation:

Organic Chemistry (Ch.25-26)

Question 73

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

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

Question 73 Explanation:

Acids & Bases (Ch. 20)

Question 74

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

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

Question 74 Explanation:

Nuclear Chemistry (Ch.28)

Question 75

Which structure below represents a ketone?

A
B
C
D
E

Question 75 Explanation:

Organic Chemistry (Ch.25-26)

Question 76

What does the symbol "ΔH" stand for?

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

Question 76 Explanation:

Thermochemistry (Ch.11)

Question 77

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

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

Question 77 Explanation:

Solutions (Ch.18)

Question 78

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

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

Question 78 Explanation:

Gas Laws (Ch.12)

Question 79

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	increasing the temperature of a solution
C	keeping the temperature of a solution constant

Question 79 Explanation:

Solutions (Ch.18)

Question 80

Which of the following is a property of an acid?

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

Question 80 Explanation:

Acids & Bases (Ch. 20)

Question 81

What is the name of the compound shown?

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

Question 81 Explanation:

Organic Chemistry (Ch.25-26)

Question 82

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

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

Question 82 Explanation:

Solutions (Ch.18)

Question 83

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

Question 83 Explanation:

Gas Laws (Ch.12)

Question 84

The bonds between adjacent water molecules are called:

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

Question 84 Explanation:

Water & Aqueous Systems (Ch.17)

Question 85

What type of acid is sulfuric acid?

A	diprotic
B	triprotic
C	protic
D	monoprotic

Question 85 Explanation:

Acids & Bases (Ch. 20)

Question 86

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

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

Question 86 Explanation:

Solutions (Ch.18)

Question 87

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

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

Question 87 Explanation:

Acids & Bases (Ch. 20)

Question 88

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	1.25 mL
C	0.5 mL
D	5.0 mL

Question 88 Explanation:

Solutions (Ch.18)

Question 89

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

A	53
B	131
C	127
D	78

Question 89 Explanation:

Nuclear Chemistry (Ch.28)

Question 90

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

Question 90 Explanation:

Solutions (Ch.18)

Question 91

The condensation of steam is a(n):

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

Question 91 Explanation:

Thermochemistry (Ch.11)

Question 92

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

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

Question 92 Explanation:

Nuclear Chemistry (Ch.28)

Question 93

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

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

Question 93 Explanation:

Thermochemistry (Ch.11)

Question 94

How many neutrons are there in an alpha particle?

A	3
B	1
C	0
D	4
E	2

Question 94 Explanation:

Nuclear Chemistry (Ch.28)

Question 95

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

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

Question 95 Explanation:

Gas Laws (Ch.12)

Question 96

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

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

Question 96 Explanation:

Nuclear Chemistry (Ch.28)

Question 97

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

Question 97 Explanation:

Thermochemistry (Ch.11)

Question 98

The structure of 2,3-dimethylheptane is:

A
B
C
D
E

Question 98 Explanation:

Organic Chemistry (Ch.25-26)

Question 99

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 99 Explanation:

Thermochemistry (Ch.11)

Question 100

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

A	neutral
B	basic
C	acidic
D	it cannot be determined

Question 100 Explanation:

Acids & Bases (Ch. 20)

Question 101

If an isotope undergoes beta emission:

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

Question 101 Explanation:

Nuclear Chemistry (Ch.28)

Question 102

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	Only small attractive and repulsive forces exists between gas particles.
D	Particles in a gas are assumed to have an insignificant volume.

Question 102 Explanation:

Gas Laws (Ch.12)

Question 103

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 103 Explanation:

Gas Laws (Ch.12)

Question 104

Which atom in a water molecule has the greatest electronegativity?

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

Question 104 Explanation:

Water & Aqueous Systems (Ch.17)

Question 105

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 increases
C	it decreases

Question 105 Explanation:

Thermochemistry (Ch.11)

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!