Unit 2 Flashcards
What factors affect gas pressure
Gas/number of particles, volume, pressure, temperature
What is a mole
6.02x10^23
What is the relation of number of particles and volume
Directly related
What is the relationship of temperature and volume
Directly related
What is the relationship with pressure and volume
Inversely related
What is relation of temp and pressure
Directly
Boyles law
P1V1=P2V2
Charles law
V1/T1=V2/T2
Guy-lussacs law
P1/T1=P2/T2
Combined gas law
P1V1/T1=P2V2/T2
Avogadros law and STP
V1/n1=V2/n2
22.4L/1mole=V2/n2
What is standard temp
273K
What is standard pressure
1 atm
Molar volume
One mile= 22.4L at STP
Dalton law of partial pressure
P1+P2+…..Pn=Ptotal
Real gases behave like ideal gases except at
Very low temps
The gas constant R is equal to .0821 when the pressure is expressed in
ATM
As more gas particles are added into a container what happens to the collisions
Increase because they don’t go as far away from one another
What is the relation of proportion for the number of Moles of a gas to its volume at STP
Number of moles is directly proportional to its volume
Real gases behave like ideal gases expect at —- pressures
Low pressures
Ideal gas equation will only give correct values if temperature is expressed in
Kalvin
One mole is how many liters
22.4
What are different units of pressure
Mm Hg Atm Pa kPa Torr
Elastic collision
Using lose velocity when collide
Ideal gas
No volume Elastic collision Constant straight line random motion Don't attract or repel AVg Kinetic energy directly related to kale in
Real gas
Volume
Attract each other
Gas behavior is most ideal at
Low pressures
High temp
Lower attractive force ( non polar)
Gases particle motion
Random no attraction
Gases have low density
No volume lots of empty space
Diffusion
Stays in container but spreads throughout
Effusion
Leaves container
Pressure formula with surface area
Force/ SA
Density formula
D= p(molar mass MM)/RT
D=m/v
P/RT=N/V or m/v
Combined gas law with avogadros law
PV/nT= R
Ideal gas law
pV=nRT
What causes effusion and deffusion
Just molecules moving and mix
What causes diffusion to happen slower or faster (rates)
Mass
