gases

dalton's law of partial pressures

states that the total pressure of a mixture of gases is equal to the sum of the artial pressures of the component gases

dalton's law formula

Ptotal = P1 + P2 + P3…

boyle's law

the volume of a fixed amount of gas varies inversely with the pressure at a constant

boyle's law formula

P1V1=P2V2

charles' law

the volume of a fixed amount of gas varies directly with the kelvin temp at constant pressure

charles' law formula

V1/T1=V2/T2

gay-lussac's law

the pressure of a fixed amount of gas varies directly with the kelvin temp. at a constant volume

gay-lussac's law formula

P1/T1=P2/T2

combined gas law

expresses the relationship between P1 T1 and V when the amount of gas is constant

combined gas law formula

P1V1/T1=P2V2/T2

molecular composition of gases

at the same temp and pressure # mols=#of liters=# of g

gay-lussac's law of combining volumes of gases

at a constant temperature and pressure the volume of gaseous reactants and products can be expresses as ratios of small whole numbers

Avogadro's Principle definition

equal volumes of gases at the same temp and pressure contain equal numbers of molecules

avogadro's principle equation

v1/n1=v2/n2, same temp and pressure vary directly with number of moles in gas

standard molar volume of gas

the volume occupied by one mole of a gas at stp and has been measured to be 22.4 liters

mole to liter conversion at STP

22.4L =1 mol

ideal gas law definition

the relationship between P,V, and T

ideal gas law

PV=nRT, MM=mRT/PV, d=PMM/Rt=T

kinetic energy formula

KE=1/2mv^2 v=velocity

KE rules

KE gas1=KE gas2

effusion and diffusion formula

v1/v2=√m2/m1

graham's law of effusion and diffusion

the rates of diffusion or effusion of gases at the same T and P are inversely proportional to the square roots of their molar masses

graham's law

rate of effusion of A/rate of effusion of B=ra/rb

kinetic molecular theory of matter

based on the idea that particles that make up matter are always in motion

KMT of gases based on assumptions

1. gases consist of large #'s of tiny particles that are far apart relative to their size
   2.collision between gas particles and between particles and the walls of the container are elastic collision
2. gas particles are in constant, rapid, random motion
3. there are no forces of attraction of repulsion between gas particles
   5.the average kinetic energies of gas particles depend on the temperature of the gas

physical properties of gases

gases expand, when temp rises volume rises, when pressure decreases volume increases, fluidity related to assumptions 3+4, low density D=m/v (volume increase density decreases), compressibilty (assumption 1,4,5,), diffusion and effusion

diffusion

sponteneous mixing of the particles of 2 substances caused by their random motion

effusion

a process by which gas particles under pressure pass through a tiny opening

ideal gas

an imaginary gas that perfectly fits all assumptions of the KMT

real gas

does not behave completely according to the assumptions of the kinetic molecular theory

pressure

defined as force per unit area on a surface P=force/area

atmopheric pressure

the sum of the individual pressured of the various gases in the atmosphere

barometer

a device used to measure atmospheric pressure. Introduced by Torricelli who found that at sea level and 0 C the average atmospheric pressure could support a 760 mm column of mercury