Chem printed notes unit Flashcards
The Kinetic Theory of Matter
all particles of matter are in motion
Kinetic theory of gases
- gases are tiny
- no definite volume and are independent
- move fast in a straight line and change direction in collision
- are elastic and don’t stick together
Kinetic energy are…
transferred but not lost
Gas pressure
collision of gas particles with each other and their container.
as collision increases
pressure increases
as temperature increases
pressure increases
altitude increases
atmospheric pressure decreases
As volume increases,
pressure decreases.
standard pressure
average pressure at sea level.
- 1 atm
- 760 mmHg
- 101.3 kPa
Kelvin
(temperatureis the amt of kenetic energy)
KE is proportional to Kelvin
Celsius + 273
Kinetic Molecular theory about gases
- movement is straight
- motion is constant and random
- no attractive/repulsive forces among particles
Factors Affecting Gas Pressure
- as the amt of gas increases, pressure increases
- as volume decreases, pressure increases
- as temp increases, pressure increases
Boyle’s law
PV=PV
Charles’ law
v/t=v/t
Gay-Lussac’s Law
p/t=p/t
the combined gas law
pv/t=pv/t
Ideal gases
gases that follow the kinetic molecular theory/gas laws (ATM IS AT A CONSTANT)
Ideal Gas Law
PV=nRT
R= .0821, pressure is in atm
Dalton
Ptotal=P1+P2+P3
Diffusion
gas particles spread
Effusion
Graham
gas escape through a small hole
When will real gas deviate from ideal gas behavior
- high pressure
- low temp
- high molar mass
- polar molecules
Intermolecular Forces (IM)
forces of attraction btw particles (more in solids)
Flow
particles can slide past eachother (only gas and liquids)
Compressible
liquid and gas but gas is more
KE
gas has more and solid has least
Viscosity:
inability to flow
Evaporation
liquid to gas below boiling point. Particles must have enough KE to beat IM. Highest KE at surface. cools overall
Evaporation in a closed container
after evaporation, particles will lose energy and become a liquid.
Equilibrium
reaction ocuring at the same rate, dynamic process bc looks likes nothing is happening
Vapor Pressure
pressure caused by evaporated particles in closed container. vapor can b measure in container
As temp increases
pressure increases
as im forces increases
vp decreases
boiling
conversion throughout substance. In order to boil, vapor pressure=atm pressure. Temp remains constant. also occurs by lowering atm pressure
normal boiling point
boiling at standard pressure (sea level)
high atm
bp increases
low atm
bp decreases
Crystaline
solid particles arranged in a pattern
Amorphous
no order in particle
Ionic (metal and nonmetal)
positive and negative, stronger higher normal boiling point
Molescular (nonmetal)
covalent bond, weaker IM
Sublimation
solid to gas without liquid. occurs when vapor pressure is greater/equal to atm
deposition
gas to solid without liquid
VP of soild
is lower than vp of a liquid
phase diagram
shows temp and pressurre
liquid state more dense than solid
slant left
Molarity (M)
Liters of solution on bottom
Molarity
Liters of solution on bottom
Molality (m)
Kg