Chemistry Exam Review 2Nd Semester

Front 1

correct value for Avogadro's number

Back 1

6.022 x 10(exponent23)

Front 2

A ____________ formula tells what elements are present and gives the simplest whole-number ration of atoms in the compound.

Back 2

empirical

Front 3

How many atoms are in 2.00kg of copper?

Back 3

2.84 x 10(exponent 24) atoms Cu

Front 4

What is the molar mass of NaCl

Back 4

58.44 g

Front 5

Which of the following is not a property of gas?

Back 5

malleability

Front 6

the coefficients of a balanced equation give molar ratios rather than mass ratios

Back 6

true

Front 7

Balanced equations are required in order to perform stoichiometric calculations correctly.

Back 7

true

Front 8

The mass of a known substance may be converted to moles using the gram-molecular mass of that substance.

Back 8

true

Front 9

The number of helium atoms in a mole of helium is equal to the number of lead atoms in a mole of lead.

Back 9

false

Front 10

Which of the following is not an assumption of the kinetic theory?

Back 10

Gas molecule lose energy when they collide with one another.

Front 11

Which property of gases best explains the fact than an ordor produced in one part of a room can soon be detected throughout the room?

Back 11

permeability

Front 12

Which of the following pairs is related by an inverse relationship?

Back 12

pressure and temperature

Front 13

Which gas law focuses on the relationship between pressure and volume?

Back 13

Boyle's law

Front 14

Which gas law is represented by the equation PV=nRT?

Back 14

ideal gas law

Front 15

The gas law that focuses on the relationship between volume and temperature is ___________________.

Back 15

Charles's law

Front 16

The volume occupied by Avogadro's number of molecules of gas at STP is known as the _____________.

Back 16

molar volume

Front 17

The gas law that focuses on the relationship between pressure and temperature is

Back 17

Gay-Lussac's law

Front 18

The volumes of reacting gases and their gaseous products are expressed in small whole numbers.

Back 18

the law of combining volumes

Front 19

What law states that the total pressure of a mixture of gases equals the sum of the partial pressures?

Back 19

Dalton's law of partial pressures

Front 20

All gas molecules of the same the have the same speed at the same temperature.

Back 20

False

Front 21

Diffusion could not occur if molecules were not in constant motion.

Back 21

True

Front 22

The abbreviation STP represents the standard conditions of 760 atm and 273K.

Back 22

false

Front 23

if the temperature of a quantity of gas changes from 100 Celsius to 200 Celsius, the volume of the gas will double if the pressure remains constant.

Back 23

false

Front 24

Charles's law is an example of a direct relationship.

Back 24

True

Front 25

The gas laws cannot be violated.

Back 25

? (it's on test 10 question 17)

Front 26

Only ideal gases actually behave according to the kinetic theory.

Back 26

true

Front 27

Gay-Lussac's law describes the observation that the pressure in hot tires is greater than it is in the same tires when they are cold.

Back 27

true

Front 28

According to the kinetic theory, gravitational, electrical, and chemical forces between molecules must be considered in addition to collisions.

Back 28

true

Front 29

Collisions constantly change the speed and direction of gas molecules.

Back 29

true

Front 30

When solving gas law equations you can use either the Celsius or Kelvin temperature scale.

Back 30

Test chapter 10 question 22 ???
answer???

Front 31

A mole of any gas will always occupy 22.4 L at STP.

Back 31

true

Front 32

A gas quickly expands to fill a low pressure region.

Back 32

expansibility

Front 33

A gas easily mingles with another porous substance.

Back 33

? Chapter 10 #24

Front 34

A gas easily mingles with another porous substance.

Back 34

? Chapter 10 #25

Front 35

Collisions of gas molecules conserve energy

Back 35

elasticity

Front 36

High pressure can squeeze gases into smaller volumes.

Back 36

compressibility

Front 37

Gas molecules move constantly to uniformly fill their containers.

Back 37

? Chapter 10 # 28

Front 38

has lower values for gases than for solids and liquids

Back 38

density

Front 39

determined by the average kinetic energy of molecules

Back 39

temperature

Front 40

depends on the force and numbers of collisions per second

Back 40

pressure

Front 41

has the same value for 1 mole of any ideal gas at STP

Back 41

volume

Front 42

For a constant quantity of gas at a constant pressure, if you decrease the temperature the volume must _____________.

Back 42

decrease

Front 43

For a constant quantity of gas at constant temperature, if you decrease the volume, the pressure will __________.

Back 43

decrease (? you might want to check to be sure test 10 question 34)

Front 44

For a given quantity of gas in a container with a fixed volume, if you increase the temperature, the pressure will ____________________.

Back 44

increase

Front 45

A solution is ____________________

Back 45

homogenous mixture

Front 46

A student desires to remove the odor of naphthalene, a nonpolar aromatic hydrocarbon, from his laboratory coat. Which solvent would you suggest?

Back 46

benzene (nonpolar)

Front 47

The rate of solution of glucose in water will NOT be increased by `

Back 47

higher pressure

Front 48

The molarity of a solute in a solution is the number of

Back 48

moles of solute per liter of solution

Front 49

When one mole of LiBr is dissolved in one kilogram of water, the concentration of the Br (with a negative sign up in the air) is

Back 49

1.0 molar

Front 50

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

Back 50

color

Front 51

Which of the following is not an example of a colloid?

Back 51

fruit punch

Front 52

A solution has a variable rather than a fixed composition

Back 52

true

Front 53

The process of separation solutes from each other involves the absorption of heat.

Back 53

? Chapter 12 number 12

Front 54

Gases are generally more soluable at higher temperatures than at lower temperatures.

Back 54

false

Front 55

Percent by mass is defined as the mass of the solute divided by the mass of the solvent multiplied by 100%.

Back 55

true.

Front 56

The abbreviation for molarity is M.

Back 56

true

Front 57

I skipped these 2 questions because they were bonus, and I didn't know if you had been given the correct answers or not.

Back 57

Chapter 12 numbers 16 & 17

Front 58

Colligative properties depend on the type, not the number, of particles in solution.

Back 58

false

Front 59

Substances that cannon be broken apart by water molecules.

Back 59

insoluble

Front 60

Two substances when mixed together do not form a solid.

Back 60

immiscible

Front 61

Addition of solutes affects the boiling point

Back 61

boiling pint elevation

Front 62

addition of solutes affects the freezing point

Back 62

freezing point elevation

Front 63

An endothermic reaction involves

Back 63

a gain of energy in the form of heat

Front 64

An exothermic reaction involves

Back 64

breaking of weaker bonds to from stronger bonds

Front 65

Which of the following has the greatest entropy?

Back 65

1 mole of NaCl (g) at 50 degrees Celsius

Front 66

According to the __________, the enthalpy change of a reaction equals the sum of the enthalpy changes for each step of the reaction.

Back 66

Hess's Law

Front 67

Thermochemistry can answer the question "Can 2 substance react together?"

Back 67

true

Front 68

Spontaneous reactions always occur rapidly.

Back 68

false

Front 69

Energy is always required to break bonds.

Back 69

true

Front 70

When ice melts, entropy increases.

Back 70

True

Front 71

The stronger the bond, the less energy released when it forms.

Back 71

false

Front 72

A reaction is favorable if the free energy change is negative.

Back 72

true

Front 73

The lower the specific heat of a substance is, the more heat will be required to cause a temperature change in the substance.

Back 73

false

Front 74

According to the laws of thermodynamics, the universe could not have formed spontaneously.

Back 74

true

Front 75

The heat that, when applied to a substance, results in bonds breaking but no temperature change.

Back 75

latent heat

Front 76

The heat that, when applied to a substance, results in a temperature change in the substance.

Back 76

sensible heat

Front 77

States that energy can be neither created nor destroyed.

Back 77

first law of thermodynamics

Front 78

An equation that combines the change in enthalpy and the change in entropy.

Back 78

Gibbs free energy

Front 79

States that natural processes decrease the order of the universe.

Back 79

collision theory

Front 80

Explains why reactions occur at greater rates, depending on reaction conditions.

Back 80

enthalpy of reeaction

Front 81

A single criterion for favorability for a reaction to occur.

Back 81

second law of thermodynamics

Front 82

The quantity represented by (a small triangle or delta sign in front of) H

Back 82

free energy

Front 83

Which of the following is a special and distinct class of catalysts comprised of naturally occurring biological substances.

Back 83

enzyme

Front 84

Solid materials that are capable of adsorbing molecules of gases or liquids onto their surfaces are called ________ catalysts.

Back 84

heterogeneous

Front 85

Any substance that changes a reaction rate without being permanently changed or consumed is called a _________________.

Back 85

catalyst

Front 86

The process of molecules of one substance collecting on the surface of another is called

Back 86

adsorption

Front 87

Rate laws are determined

Back 87

experimentally

Front 88

Doubling the concentration of a reactant always causes the reaction rate to double.

Back 88

false

Front 89

Spontaneous reactions always occur rapidly.

Back 89

false

Front 90

A catalyst does not affect the concentration of products formed in a reaction; it only affects the rate at which they are produced.

Back 90

true

Front 91

A reaction that has a large activation energy is more likely to occur than a reaction with a low activation energy.

Back 91

false

Front 92

Any factor that increases the number of effective collisions increases the reaction rate.

Back 92

true

Front 93

A rate law with a specific rate constant allows you to calculate how fast a reaction will occur.

Back 93

true

Front 94

A thermodynamically favorable reaction proceeds spontaneously.

Back 94

false

Front 95

Indicates how the rate of a reaction is affected by a specific reactant's concentration

Back 95

reaction order

Front 96

the study of the rates of reaction and the steps by which they occur

Back 96

kinetics

Front 97

the minimum amount of kinetic energy that must be possessed by reactants before they can react

Back 97

activation energy

Front 98

a theoretical, unstable, high-energy, transitional substance in a reaction

Back 98

activated complex

Front 99

usually tells how fast reactants change into products

Back 99

reaction rate

Front 100

the series of steps that make up a reaction

Back 100

reaction mechanism

Front 101

an equation that mathematically describes how fast a reaction can occur

Back 101

rate law

Front 102

explains why reaction occur at greater or slower rates, depending on reaction conditions

Back 102

collision theory

Front 103

What states than when an equilibrium is stressed, it will proceed in the direction that will relieve the stress?

Back 103

Le Chatelier's principle

Front 104

Once a chemical system reaches equilibrium, there is no further reaction between the particles of the reactants and the products.

Back 104

true (check chapter 15 # 13)

Front 105

An increase in temperature favors the exothermic reaction in an equilibrium reaction.

Back 105

true (check chapter 15 # 14)

Front 106

Adding a catalyst changes the value of the equilibrium constant

Back 106

true ((check chapter 15 # 15)

Front 107

If the produce of the concentrations of the ions making up the solution is greater than the K(with a subscript sp) for the precipitate, the solution is supersaturated.

Back 107

true

Front 108

Le Chatelier's principle indicates that when the equilibrium of a reaction is disturbed,it reacts to minimize the disturbance.

Back 108

true

Front 109

When the pressure of a system in equilibrium is decreased, the system will favor the direction of the smaller number of moles of gas to reestablish equilibrium.

Back 109

false

Front 110

There are quite a few questions from test chapter 15 that I could not type.

Back 110

There are quite a few questions from test chapter 15 that I could not type.

Front 111

At 25 degrees Celcius, what does the pH + the pOH equal

Back 111

0

Front 112

A neutralization reaction produces both water and

Back 112

? Chapter 15 (it says 15 but I think it's really 16) number 5

Front 113

The strength of an acid is determined by

Back 113

how many types of particles are in the solution

Front 114

What do indicators tell?

Back 114

the pH of a solution

Front 115

Why would you do a titration?

Back 115

to determine if a buffer should be used

Front 116

The Lewis definitions deal with an acid donating or taking protons.

Back 116

false ? it says 15 but I think it's really 16 # 11)

Front 117

Buffers help to maintain a neutral pH.

Back 117

false

Front 118

Acids taste sour.

Back 118

true

Front 119

When acids lose protons, it is called protonation.

Back 119

false

Front 120

If an acid is strong, its conjugate base must be weak.

Back 120

true

Front 121

All Arrhenius acids are Bronsted-Lowry acids.

Back 121

true

Front 122

When sulfur changes from an oxidation state of -2 to +6 in the sulfate ion, the sulfur must

Back 122

lose 8 electrons

Front 123

The gaining of electrons by an ion or atom is

Back 123

reduction

Front 124

The losing of electrons by an ion or atom is

Back 124

oxidation

Front 125

All of the following changes in oxidation represent oxidation with the exception of

Back 125

-1 to -3

Front 126

An oxidizing agent is a substance that

Back 126

supplies electrons

Front 127

Oxidation reaction always involve the element oxygen.

Back 127

false

Front 128

Redox reactions can occur only when electrons are transferred between metals and nonmetals.

Back 128

false

Front 129

Oxidation and reduction are simultaneous reactions.

Back 129

true

Front 130

In redox reactions, the reducing agent gains electrons.

Back 130

false