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School > Chemistry - Trimester 3 Final > Flashcards

Chemistry - Trimester 3 Final Flashcards

1
Q

compressibility

A

a measure of how much the volume of matter decreases under pressure

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2
Q

Boyle’s Law

A

P1V1 = P2V2

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3
Q

Charle’s Law

A

V1/T1 = V2/T2

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4
Q

Gay-Lussac’s Law

A

P1/T1 = P2/V2

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5
Q

combined gas law

A

P1V1/T1 = P2V2/T2

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6
Q

ideal gas constant

A

R = 8.31 ( L x kPa)/(K x mol)

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7
Q

ideal gas law

A

PV = nRT

it describes the behavior of the gas

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8
Q

partial pressure

A

the contribution each gas in a mixture of gases makes to the total pressure

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9
Q

Dalton’s Law of partial pressure

A

at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases

Ptotal = P1 + P2 + P3 + … etc…

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10
Q

diffusion

A

the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout

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11
Q

effusion

A

process that occurs when a gas escapes through a tiny hole in its container

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12
Q

Graham’s Law of effusion

A

square root of… molar mass of B / molar mass of A

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13
Q

aqueous solution

A

water that contains dissolved substances

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14
Q

solvent

A

dissolving medium in a solution

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15
Q

solute

A

dissolved particles in a solution

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16
Q

solvation

A

a process that occurs when an ionic solute dissolves

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17
Q

electrolyte

what are electrolytes?

A

a compound that conducts an electric current when it is in an aqueous solution or in the molten state

ionic compounds

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18
Q

nonelectrolyte

A

a compound that does not conduct an electric current in aqueous solution or in the molten state

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19
Q

strong electrolyte

A

a solution in which a large portion of the solute exists as ions

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20
Q

weak electrolyte

A

a solution that conducts electricity poorly because only a fraction of the solute exists as ions

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21
Q

water of hydration

A

water molecules that are an integral part of a crystal structure

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22
Q

hydrate

A

a compound that has a specific number of water molecules bound to each formula unit

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23
Q

anhydrous

A

describes a substance that does not contain water

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24
Q

effloresce

A

to lose water of hydration; the process occurs when the hydrate has a vapor pressure higher than that of water vapor in the air

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25
Q

hygroscopic

A

a term describing salts and other compounds that remove moisture from the air

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26
Q

desiccant

A

a hygroscopic used as a drying agent

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27
Q

deliquescent

A

describes a substance that removes sufficient water from the air to form a solution; the solution

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28
Q

saturated solution

A

a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure

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29
Q

solubility

A

the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution

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30
Q

unsaturated solution

A

a solution that contains less solute than a saturated solution at a given temperature and pressure

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31
Q

miscible

A

describes liquids dissolve in one another in all proportions

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32
Q

immiscible

A

describes liquids that are insoluble in one another

ex. oil and water

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33
Q

supersaturated solution

A

a solution that contains more solute than it can theoretically hold at a given temperature

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34
Q

Henry’s Law

A

states that at a given temp., the solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas above the liquid

S1/P1 = S2/P2

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35
Q

concentration

A

a measurement of the amount of solute that is dissolved in a given quantity of solvent, usually expressed as mol/L

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36
Q

dilute solution

A

a solution that contains a small amount of solute

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37
Q

concentrated solution

A

a solution containing a large amount of solute

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38
Q

molarity (M)

A

moles of solute / 1 liter of solution

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39
Q

thermochemistry

A

the study of energy changes that occur during chemical reactions and changes in state

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40
Q

chemical potential energy

A

energy stored in chemical bonds

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41
Q

heat

A

(q) energy that transfers from one object to another because of a temperature difference between the objects

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42
Q

system

A

a part of the universe on which you focus your attention

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43
Q

surroundings

A

everything in the universe outside of the system

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44
Q

law of conservation of energy

A

no energy created nor destroyed

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45
Q

endothermic process

A

process that absorbs heat from the surroundings

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46
Q

exothermic process

A

process that releases heat to its surroundings

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47
Q

heat capacity

A

amount of heat needed to increase the temperature of an object exactly 1°C

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48
Q

specific heat

A

the amount of heat needed to increase the temperature of 1g of a substance 1°C

also called specific heat capacity

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49
Q

calorimetry

A

the precise measurement of heat flow out of a system for chemical and physical processes

50
Q

calorimeter

A

an insulated device used to measure the absorption or release of heat in chemical or physical processes

51
Q

enthalpy

A

(H) the heat content of a system at constant pressure

52
Q

thermochemical equation

A

a chemical equation that includes the enthalpy change

53
Q

heat of reaction

A

the enthalpy change for a chemical exchange exactly as it is written

54
Q

heat of combustion

A

the heat of reaction for the complete burning of one mole of a substance

55
Q

molar heat of fusion

A

S –> L

56
Q

molar heat of solidification

A

L –> S

57
Q

molar heat of vaporization

A

L –> G

58
Q

molar heat of condensation

A

G –> L

59
Q

molar heat of solution

A

the enthalpy change caused by the dissociation of one mole of a substance

60
Q

rate

A

describes the speed of change over an interval of time

61
Q

collision theory

A

atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy

62
Q

activation energy

A

the minimum energy colliding particles must have in order to react

63
Q

activated complex

A

an unstable arrangement of atoms that exists momentarily at the peak of the activation energy barrier

called transition state

64
Q

inhibitor

A

a substance that interferes with the action of a catalyst

65
Q

reversible reaction

A

a reaction in which the conversion of reactants into products and the conversion of products into reactants occur simultaneously

66
Q

Le Chatelier’s Principle

A

when a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress

67
Q

chemical equilibrium

A

a state of balance in which the rates of the forward and reverse reactions are equal

68
Q

equilibrium position

A

the relative concentrations of reactants and products of a reaction that has reached equilibrium

69
Q

equilibrium constant

A

(Keq) the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in one balanced chemical equation

70
Q

hydronium ion

A

(H3O) the positive ion formed when a water molecule gains a hydrogen ion

71
Q

conjugate acid

A

particle formed when a base gains a hydrogen ion

72
Q

conjugate base

A

the particle that remains when an acid has donated a hydrogen ion

73
Q

conjugate acid-base pair

A

two substances that are related by the loss or gain of a single hydrogen ion

74
Q

amphoteric

A

a substance that can act as both an acid and a base

75
Q

self-ionization

A

a term describing the reaction in which two water molecules react to produce ions

76
Q

neutral solution

A

an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal

has a pH of 7.0

77
Q

ion-product constant for water (Kw)

A

[H+][OH-] = 1 x 10^-14

78
Q

acidic solution

A

any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration

79
Q

basic solution

A

any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration

80
Q

pH (3)

A

number used to denote the acidity of a substance

  • 6 and under = acid
  • 8 and higher = base
81
Q

strong acid

A

an acid that is completely (or almost completely) ionized in aqueous solution

82
Q

weak acid

A

an acid that is only slightly ionized in aqueous solution

83
Q

acid dissociation constant (Ka)

A

the ratio of the concentration of the dissociated form of an acid to the undissociated form

84
Q

strong base

A

a base that completely dissociates into metal ions and hydroxide ions in aqueous solution

85
Q

weak base

A

a base that reacts with water to form the hydroxide ion and the conjugate acid of the base

86
Q

base dissociation constant (Kb)

A

(Kb) the ratio of the concentrations of the conjugate acid times the concentration of the hydroxide ions to the concentration of the base

87
Q

neutralization reaction

A

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

88
Q

titration

A

process used to determine the concentration of a solution in which a solution of known concentration is added to a measured amount of the solution of unknown concentration until an indicator signals the end point

89
Q

standard solution

A

a solution of known concentration used in carrying out titration

90
Q

equivalence point

A

the point in a titration where the number of moles of hydrogen ions equals the number of moles of hydroxide ions

91
Q

end point

A

the point in a titration at which the indicator changes color

92
Q

How to find [H+]

A

[H+] = 10^-pH

93
Q

How to find [OH-]

A

10^-pOH

94
Q

How to find pH

A

pH = -log [H+]

95
Q

How to find pOH

A

pOH = -log [OH-]

96
Q

__ + __ = 14

A

pH + pOH = 14

97
Q

3 factors that affect gas pressure?

A

amount of gas (concentration)

volume (in liters)

temperature (T in kelvins)

98
Q

Real Gas vs Ideal Gas

A

Real - actual gas, high pressures, low temps

99
Q

how to find the number of moles of the gas?

A

use the ideal gas law – PV = nRT

100
Q

What does STP stand for?

what are STP conditions

A

Standard Temperature and Pressure

Standard Temp = 0°C (273K)
Standard Pressure = 1atm (760mmHg or 760 torr)

101
Q

what substances dissolve most readily in water

A

ionic compounds and polar covalent bonds

102
Q

why are all ionic compounds electrolytes?

A

because they dissociate into ions

103
Q

% by mass H2O =

A

mass of water / mass of hydrate (ex. 5H20, 5 x mass of H2O) x 100%

104
Q

what factors affect how fast a substance dissolves? (3)

A

agitation (rate of stirring/shaking)
temperature
particle size of solute (surface area)

105
Q

What factors affect the solubility of a substance?

A

temperature affects solubility of solid, liquid, and gases

temp and pressure affects the solubility of gaseous solutes

106
Q

Percent by volume formula

A

volume of solute / volume of solution x 100%

107
Q

Percent by mass formulas

A

mass of solute / mass of solution x 100%

108
Q

how to find the specific heat of a substance

A

q / m x △T

units = J/(g°C)

109
Q

Energy

A

heat transfer or work

110
Q

what two factors does the heat capacity of an object depend on? (2)

A

its mass and chemical composition

111
Q

factors that affect the rate of a chemical reaction (4)

A

temperature

concentration

particle size

use of a catalyst

112
Q

stressors that upset the equilibrium of a chemical system (3)

A

changes in concentration

changes in temp

changes in pressure

113
Q

what is used to measure pH (2)

A

pH meters

acid-base indicators

114
Q

kinetic molecular theory (3)

A
  1. particles in a gas are considered to be small, hard spheres with an insignificant volume
  2. the motion of the particles in a gas is rapid, constant, and random
  3. all collisions b/t particles in a gas are perfectly elastic
115
Q

solutions are…

A

homogeneous mixtures

stable

116
Q

When Keq has a large value such as …?

A

3.1 x 10^11, the reaction mixture at equilibrium will consist mainly of product

117
Q

When Keq has a small value such as…?

A

3.1 x 10^-11, the mixture at equilibrium will consist mainly of reactant

118
Q

What value would Keq be at an intermediate value? (2)

what does it mean?

A

0.15 or 50

there is a significant amount of both reactant and product

119
Q

Arrhenius definition of an acid and a base? (2)

A

acids = hydrogen-containing compounds that ionize to yield hydrogen ions (H+)

base = compounds that ionize to yield hydroxide ions (OH-)

120
Q

Bronsted Lowry definition of an acid and a base

A

acid = hydrogen-ion donor

base = hydrogen-ion acceptor

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