Chemistry all year, continously add

KMT Statement 1

Gases are tiny and spaced far apart

KMT Statement 2

Constantly and randomly moving

KMT Statement 3

Collisions are elastic (No energy transferred or lost)

KMT Statement 4

No forces of attraction or repulsion

KMT Statement 5

Kinetic energy of a gas is based on temperature

Pressure

force per area: particles hitting sides of the container

Torr conversions to 1 atm

760.

mmHg conversions to 1 atm

760

kPa conversions to 1 atm

101.3

When the mercury near the outside of the manometer is lower

Pgas=Pair-h

When the mercury near the outside of the manometer is higher

Pgas=Pair+h

Pressure of gas in a mixture…

can be measured as if it were alone

Ptot=

Pgas1+P2+P3…

Two flask problem combines?

Particle Pressures (Ptot=…) & Boyle’s law (P1V1=P2V2)

Kinetic Energy formula

3/2RT

R=8.314 J/mol*k

Root Mean Square Velocity formula

square root (3RT/MM)

R=8.314 J/mol*k

MM=kg/mol

Units: m/s

Effusion definition

Passage of gas through tiny opening into a vacuum

Effusion forumla

rate of gas1/rate of gas2 = square root (MM2/MM1)

Rate= vol/time

Diffusion definition

spreading out from high to low concentration

Diffusion graphs explained

1. number of gas molec. being larger at beginning but as velocity goes on increasing means it is heavier and small number of gas molec. at the beginning but larger as velocity increases is ligher

2. number of gas molec. being larger at beginning but as velocity goes on increasing means temperature is low and small number of gas molec. at the beginning but larger as velocity increases is higher temp

Mole Fraction definition

Mixture of gases

Mole Fraction 2 equations

Xa=na/ntot

Pa=Xa*Ptot

Density=

mass/volume

MM=

m/n

PV=

nRT

Gases behave ideally at?

high temps & low pressures