Chemistry - Trimester 3 Final Flashcards
1
Q
compressibility
A
a measure of how much the volume of matter decreases under pressure
2
Q
Boyle’s Law
A
P1V1 = P2V2
3
Q
Charle’s Law
A
V1/T1 = V2/T2
4
Q
Gay-Lussac’s Law
A
P1/T1 = P2/V2
5
Q
combined gas law
A
P1V1/T1 = P2V2/T2
6
Q
ideal gas constant
A
R = 8.31 ( L x kPa)/(K x mol)
7
Q
ideal gas law
A
PV = nRT
it describes the behavior of the gas
8
Q
partial pressure
A
the contribution each gas in a mixture of gases makes to the total pressure
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…
10
Q
diffusion
A
the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
11
Q
effusion
A
process that occurs when a gas escapes through a tiny hole in its container
12
Q
Graham’s Law of effusion
A
square root of… molar mass of B / molar mass of A
13
Q
aqueous solution
A
water that contains dissolved substances
14
Q
solvent
A
dissolving medium in a solution
15
Q
solute
A
dissolved particles in a solution
16
Q
solvation
A
a process that occurs when an ionic solute dissolves
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
18
Q
nonelectrolyte
A
a compound that does not conduct an electric current in aqueous solution or in the molten state
19
Q
strong electrolyte
A
a solution in which a large portion of the solute exists as ions
20
Q
weak electrolyte
A
a solution that conducts electricity poorly because only a fraction of the solute exists as ions
21
Q
water of hydration
A
water molecules that are an integral part of a crystal structure
22
Q
hydrate
A
a compound that has a specific number of water molecules bound to each formula unit
23
Q
anhydrous
A
describes a substance that does not contain water
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
25
hygroscopic
a term describing salts and other compounds that remove moisture from the air
26
desiccant
a hygroscopic used as a drying agent
27
deliquescent
describes a substance that removes sufficient water from the air to form a solution; the solution
28
saturated solution
a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure
29
solubility
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
30
unsaturated solution
a solution that contains less solute than a saturated solution at a given temperature and pressure
31
miscible
describes liquids dissolve in one another in all proportions
32
immiscible
describes liquids that are insoluble in one another
ex. oil and water
33
supersaturated solution
a solution that contains more solute than it can theoretically hold at a given temperature
34
Henry's Law
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
35
concentration
a measurement of the amount of solute that is dissolved in a given quantity of solvent, usually expressed as mol/L
36
dilute solution
a solution that contains a small amount of solute
37
concentrated solution
a solution containing a large amount of solute
38
molarity (M)
moles of solute / 1 liter of solution
39
thermochemistry
the study of energy changes that occur during chemical reactions and changes in state
40
chemical potential energy
energy stored in chemical bonds
41
heat
(q) energy that transfers from one object to another because of a temperature difference between the objects
42
system
a part of the universe on which you focus your attention
43
surroundings
everything in the universe outside of the system
44
law of conservation of energy
no energy created nor destroyed
45
endothermic process
process that absorbs heat from the surroundings
46
exothermic process
process that releases heat to its surroundings
47
heat capacity
amount of heat needed to increase the temperature of an object exactly 1°C
48
specific heat
the amount of heat needed to increase the temperature of 1g of a substance 1°C
also called specific heat capacity
49
calorimetry
the precise measurement of heat flow out of a system for chemical and physical processes
50
calorimeter
an insulated device used to measure the absorption or release of heat in chemical or physical processes
51
enthalpy
(H) the heat content of a system at constant pressure
52
thermochemical equation
a chemical equation that includes the enthalpy change
53
heat of reaction
the enthalpy change for a chemical exchange exactly as it is written
54
heat of combustion
the heat of reaction for the complete burning of one mole of a substance
55
molar heat of fusion
S --> L
56
molar heat of solidification
L --> S
57
molar heat of vaporization
L --> G
58
molar heat of condensation
G --> L
59
molar heat of solution
the enthalpy change caused by the dissociation of one mole of a substance
60
rate
describes the speed of change over an interval of time
61
collision theory
atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy
62
activation energy
the minimum energy colliding particles must have in order to react
63
activated complex
an unstable arrangement of atoms that exists momentarily at the peak of the activation energy barrier
called transition state
64
inhibitor
a substance that interferes with the action of a catalyst
65
reversible reaction
a reaction in which the conversion of reactants into products and the conversion of products into reactants occur simultaneously
66
Le Chatelier's Principle
when a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress
67
chemical equilibrium
a state of balance in which the rates of the forward and reverse reactions are equal
68
equilibrium position
the relative concentrations of reactants and products of a reaction that has reached equilibrium
69
equilibrium constant
(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
hydronium ion
(H3O) the positive ion formed when a water molecule gains a hydrogen ion
71
conjugate acid
particle formed when a base gains a hydrogen ion
72
conjugate base
the particle that remains when an acid has donated a hydrogen ion
73
conjugate acid-base pair
two substances that are related by the loss or gain of a single hydrogen ion
74
amphoteric
a substance that can act as both an acid and a base
75
self-ionization
a term describing the reaction in which two water molecules react to produce ions
76
neutral solution
an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal
has a pH of 7.0
77
ion-product constant for water (Kw)
[H+][OH-] = 1 x 10^-14
78
acidic solution
any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration
79
basic solution
any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration
80
pH (3)
number used to denote the acidity of a substance
- 6 and under = acid
- 8 and higher = base
81
strong acid
an acid that is completely (or almost completely) ionized in aqueous solution
82
weak acid
an acid that is only slightly ionized in aqueous solution
83
acid dissociation constant (Ka)
the ratio of the concentration of the dissociated form of an acid to the undissociated form
84
strong base
a base that completely dissociates into metal ions and hydroxide ions in aqueous solution
85
weak base
a base that reacts with water to form the hydroxide ion and the conjugate acid of the base
86
base dissociation constant (Kb)
(Kb) the ratio of the concentrations of the conjugate acid times the concentration of the hydroxide ions to the concentration of the base
87
neutralization reaction
a reaction in which an acid and a base react in an aqueous solution to produce a salt and water
88
titration
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
standard solution
a solution of known concentration used in carrying out titration
90
equivalence point
the point in a titration where the number of moles of hydrogen ions equals the number of moles of hydroxide ions
91
end point
the point in a titration at which the indicator changes color
92
How to find [H+]
[H+] = 10^-pH
93
How to find [OH-]
10^-pOH
94
How to find pH
pH = -log [H+]
95
How to find pOH
pOH = -log [OH-]
96
__ + __ = 14
pH + pOH = 14
97
3 factors that affect gas pressure?
amount of gas (concentration)
volume (in liters)
temperature (T in kelvins)
98
Real Gas vs Ideal Gas
Real - actual gas, high pressures, low temps
99
how to find the number of moles of the gas?
use the ideal gas law -- PV = nRT
100
What does STP stand for?
what are STP conditions
Standard Temperature and Pressure
Standard Temp = 0°C (273K)
Standard Pressure = 1atm (760mmHg or 760 torr)
101
what substances dissolve most readily in water
ionic compounds and polar covalent bonds
102
why are all ionic compounds electrolytes?
because they dissociate into ions
103
% by mass H2O =
mass of water / mass of hydrate (ex. 5H20, 5 x mass of H2O) x 100%
104
what factors affect how fast a substance dissolves? (3)
agitation (rate of stirring/shaking)
temperature
particle size of solute (surface area)
105
What factors affect the solubility of a substance?
temperature affects solubility of solid, liquid, and gases
temp and pressure affects the solubility of gaseous solutes
106
Percent by volume formula
volume of solute / volume of solution x 100%
107
Percent by mass formulas
mass of solute / mass of solution x 100%
108
how to find the specific heat of a substance
q / m x △T
units = J/(g°C)
109
Energy
heat transfer or work
110
what two factors does the heat capacity of an object depend on? (2)
its mass and chemical composition
111
factors that affect the rate of a chemical reaction (4)
temperature
concentration
particle size
use of a catalyst
112
stressors that upset the equilibrium of a chemical system (3)
changes in concentration
changes in temp
changes in pressure
113
what is used to measure pH (2)
pH meters
acid-base indicators
114
kinetic molecular theory (3)
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
solutions are...
homogeneous mixtures
stable
116
When Keq has a large value such as ...?
3.1 x 10^11, the reaction mixture at equilibrium will consist mainly of product
117
When Keq has a small value such as...?
3.1 x 10^-11, the mixture at equilibrium will consist mainly of reactant
118
What value would Keq be at an intermediate value? (2)
what does it mean?
0.15 or 50
there is a significant amount of both reactant and product
119
Arrhenius definition of an acid and a base? (2)
acids = hydrogen-containing compounds that ionize to yield hydrogen ions (H+)
base = compounds that ionize to yield hydroxide ions (OH-)
120
Bronsted Lowry definition of an acid and a base
acid = hydrogen-ion donor
base = hydrogen-ion acceptor
