UNIT FIVE Flashcards
kinetic-molecular theory of gases
particles of matter are always in motion
ideal gas
imaginary gas that perfectly fits all assumptions of kinetic-molecular theory
assumptions of kinetic-molecular theory
1) gases consist of many tiny particles that are far apart
2) collisions between gas particles, particles, container walls are elastic (no net loss of kinetic energy)
3) in constant, rapid motion
4) no forces of attraction/repulsion between particles
5) average kinetic energy of gas particles depends on temperature (KE=1/2 mass x speed)
expansion
fills container
fluidity
gas particles slide easily due to few attractive forces
low density
particles very far apart
compressibility
initially far apart can be pushed together
diffusion
spontaneous mixing of particles of 2 substances caused by random motion and depends on particle speed, diameter, attractive forces
effusion
process where gas particles under pressure pass through tiny openings and is directly proportional to particle velocity
barometer
measures atmospheric pressure
Boyle’s Law
P1V1 = P2V2
Charles’ Law
V1/T1 = V2/T2
Gay-Lussac’s Law
P1/T1 = P2/T2
Combined Law
(P1V1)/T1 = (P2V2)/T2
Ideal Gas Law
PV = nRT
Avogadro’s Law
equal volume of gases at the same temperature and pressure has the same number of molecules
gas standard molar volume
volume occupied by 1 mole of gas at standard temperature and pressure
Graham’s Law of Effusion
rate of effusion of gases at same temperature and pressure are inversely proportional to their square root molar masses
liquid
form of matter that has definite volume and takes shape of container
fluid
substance that can flow and take the shape of its container
properties of liquids
- relatively high density
- relative incompressibility
- ability to diffuse
- surface tension
- evaporation
- boiling
crystalline solids
consists of many crystal (most solids) and particles are pattered orderly, geometric and repeating
amorphous solids
particles arranged randomly such as plastic and gas
equilibrium
dynamic condition where two opposite charges occur at closed rates in equal rates
Le-Chatelier’s Principle
when equilibrium system is disturbed y application of stress, it attains new equilibrium that minimizes stress
volatile liquids
liquids that evaporate easily
molar heat of vaporaization
energy required to vaporize one mole of liquid at boiling point, high when intermolecular forces are strong
molar heat of fusion
energy required to melt one mole of solid at melting point
phase diagrams
graph of pressure versus temperature, shows conditions under which phases exist
triple point of a substance
indicates temperature and pressure conditions when solid, liquid, and vapour coexist at equilibrium
solution
uniform mixture of two or more substances
solvent
component of a solution present in largest amount
solute
components of solution present in smaller amounts than solvent
solute
components of solution present in smaller amounts than solvent
electrolyte
substance that dissolves in water and creates conductive solution, includes all soluble ionic compounds and highly polar molecular compounds
nonelectrolyte
dissolves but does not create conductivity, eg sugar
solution equilibrium
physical state in which opposing process of dissolution and crystallization occur at equal rates
saturated solution
contains maximum amount of dissolved solute
supersaturated solution
contains more dissolved solute in same conditions
Henry’s Law
solubility of gas in a liquid is directly proportional to partial pressure of that gas on surface of liquid
molality
amount of solute (moles, n) divided by mass (m) of solvent in kg
m=n/m
molarity
amount of solute divided by volume
M=n/V
