Gas Laws

solids movement

atoms and molecules vibrate but don’t move around

liquids movement

atoms move around but stay tg

gas movement

atoms and molecules move and spread apart

gas pressure

pressure from gas particles moving and colliding with surfaces

what is gas pressure dependent on

of gas particles in a given volume

volume of the container

avg speed of gas particles

quantitative physical properties of gasses

pressure (P)

volume (V)

temp (T)

amount in moles (n)

simple gas laws

describes relatinoship btwn pairs of these properties

what are simple gas laws explained thru

kinetic molecular theory

kinetic molecular theory of gases

describes ideal or theoretical behavior of gases

what does kinetic molecular theory of gas state

molecules of gas are in constant motion causing collision with walls that cause pressure

most of the space between particles is empty, so volume of molecules is negligable

particles do not attract or repel one another

ideal gasses have no itnermolecular force

what properties does boyle’s law involve

pressure and volume

what is boyle’s law

volume of a fixed quantity of gas at constant temp is inversely prop to the pressure

p and va re inversely prop

how is boyle’s law plotted

hyperbola/curve

charles' law

v of a fixed mass of gas is directly prop to k temp if v is constatn

avogadro’s law

volume of gas is prop to number of moles

ideal gas law

PV=nRT

what does the units nad values for R depend on

units of P and V

why aren’t the units for R dependent on T

T is always in kelvins

molar volume

the volume of 1 mol of any gas at STP

STP

273.15K, or 0C, and P=1 atm

same number of mols but mass is diff

what does PV=nRT describe

ideal gas behavior

attractive forces btwn ideal gas molecuels are negligable

how do gasses mix

they mxi well in any proportion

in a solution of gasses, it is assumed each gas behaves independently

partial pressure of gasses

in a mixture of gas, the partial pressure is the pressure that one gas would exert if it occupied the container by itself

dalton’s law of partial pressure

total presure of a mixture of non reacting gases is equal to the sum of pressures that would exert if it were present alone

dalton’s law of partial pressure as an equation

Ptotal = P1 + P2 + P3 etc

mole fraction (X)

gives portion fo the total pressure that is contributed by a specific gas

alternate def of mole fraction

ratio of number of moles of a gas to total number of mols in teh mixtures

mole percent

molef raction x 100

vapor

gas form of a substance that is usually a liquid or solid at room temp

type of gas

vapor pressure

pressure of vapor over liquid

when you collect gas over water, there is al ways vapor mixed with it

what affects VP

strenght of IMF

temperature

relationship between IMF and VP

lower IMF → higher VP

relation btwn temp and VP

higher temp → higehr VP

does volume of container affect VP?

no, the volume of a container does not affect VP

P total equation for vapor over a liquid

Ptotal = Pgas + Pvapor

what phases can form vapor

solids and liquids

what phase are all ionic compounds at room temp

solid

how does temperature impact KE

at the same temperature, two different substances would still have the same kinetic energy

how does mass impact speed of molecule

higher mass → lower velocity

KE=1/2mv²

if KE is the same for both substances, and mass is higher for one, then v will be lower to make it equal

diffusion

mixing of gases by dispersion from region of hgih concentration to low

effusion

escape of gas molecules through a small hole

garaham’s law of effusion

thehigher the molar mass, the lower the rate of effusion and diffusion

ideal gas

a theoretical gas that follows gas laws (PV=nRT)

properties of ideal gas

has no volume

no intermolecular forces of attraction

real gas

molecules of real gas which occupy space and exhibit attraction

under what conditions do real gasses behave ideally

high temp, lower pressure

under what. conditions can real gas overcome intermolcular forces

higher temp→higher KE

what does lowered pressure cause in real gas

behaves more ideally

more volume → more space to overcome IMFG

relationship between molar mass and ideal behavior

the greater the molar mass, the greater the deviation from ideal behavior

bc larger molecule → higher LDF