Chemistry Final

Front 1

Kinetic Molecular Theory

Back 1

1.Gas molecules are dimensionless points 2.temperature is an indirect measure of molecular kinetic energy (higher temp = faster rxn) 3. Gas mlcls are in canstant, random, straighty- line motion 4. Gas mlcls collide w/ each other and the container walls with no loss of energy 5. Gas mlcls exert no attractice/ repulsive force on on another

Front 2

Pressure

Back 2

ration of force exerted divided by the surface area over which the force is done
- force is caused by collisions
- barometer and manometer
* Pv= nRT

Front 3

Combined Gas Law Equation

Back 3

* P1V1/n1T1 = P2V2/n2T2
-Rigid container- neither expands or contracts, initial and final volumes equal
-Closed System- nothing in, nothing out, initial and final moles equal
-Insothermal- constant temp.
-cancel out variables that don't change in the problems

Front 4

Boyle's Law

Back 4

-if you study the P and V of a gas, you get Boyle's Law: * P1V1= P2V2
(smaller volume= higher pressure)

Front 5

Charles' Law

Back 5

-Shows relationship between V and T of a gas
-provides basis for concept of absolute zero (0= 0 volume)
* V1/T1 = V2/T2

Front 6

Avogadro's Principle

Back 6

-When you study the volume and moles of a gas
* V1/n1 = V2/n2

Front 7

Dalton's Law of Partial Pressures

Back 7

-if you have a mixture of gases, then the total pressure is simply equal to the sum of each of the individual partial pressures
* Ptot= Pn
-add the gase pressures together if they are simply combined in a container

Front 8

Molecular Speed

Back 8

-gas mlcls are in constant motion, but do not travel at one constant speed
-temp and molar mass effect speed
-Boltzmann Distribution- at higher temps. the curve flattens out more and stretches
*Urms = square root of 3RT/M

Front 9

Effusion and Diffusion

Back 9

-Effusion- escape of a gas through a small hole
-Diffusion- spreading of one gas through another
* U1/U2 =square root of m2/m1
-to compare rates of diffusion or effusion