gases Flashcards
1
Q
kinetic molecular theory
A
- tiny particles a long way apart (weak dispersion forces)
- volume is negligible compared to volume of container
- move rapidly in straight lines
- collisions are elastic- don’t run out of energy
- average kinetic energy of different gases is the same at the same temp
- increase temp, increase energy
2
Q
graph of kinetic energy
A
more under peak = more particles
3
Q
pressure conversions
A
750mmHg —> 0.987atm —-> 100 000 Pa —-> 100kPa —-> 1 bar
4
Q
Boyle’s law
A
as volume decreases, pressure increases and vice versa
(only applicable if temp is constant)
PV = k
P1V1 = P2V2
5
Q
Charles’ law
A
as temperature increases, so does volume of gas this is because they move faster and collide more vigorously
(pressure is constant)
6
Q
kelvins
A
c + 273
7
Q
amount of gas
A
the amount of gas is proportional to volume of gas present
pressure and temp as constant
8
Q
general gas equation
A
PV = nRT
- pressure in kPA
- volume in L
- Temp in k
- R = 8.31
- n is mol
9
Q
SLC
A
100 kPA and 25 degrees
Vm is 24.8Lmol-1
10
Q
STP
A
100kPA and 0 degrees
Vm is 22.8
11
Q
if given conditions?
A
V = n x Vm
