Gases Flashcards
1
Q
STP Values
A
- P= 101.325 kPa
- Temp = 0C = 273.15K
- Vm = 22.4 L/mol
2
Q
SATP Values
A
- P = 100kPa
- Temp = 25C = 298.15K
- Vm = 24.8 L/mol
3
Q
Pressure conversions (mmHg, atm, kPa)
A
760 mmHg = 101.325 kPa = 1 atm
4
Q
Boyles Law
A
- Inverse relationship between pressure n volume (increased P = decreased V)
- P1V1 = P2V2
5
Q
Charles Law
A
- Relationship between Temp. n Volume
- Temp increase = faster molecules = more volume
- V1 / T1 = V2 / T2
6
Q
Combined Gas Law
A
- Relationship between temp, vol, and pressure
- ( P1 x V1 )/T1 = ( P2 x V2)/ T2
7
Q
Kinetic Molecular Theory
A
- Matter is composed of small particles, volume that the particles occupy is space inbetween molecules, not what the molecules contain themselves
- Molecules are in constant random motion
- When molecules collide, there is no loss of energy
8
Q
Avogadro’s Theory
A
- Equal volumes of gases at the same time and pressure contain equal # of molecules
- Linear Relationship (vol increase = molecules increase)
9
Q
Ideal Gas Law
A
- Gas molecules are very far apart compared to size; particle size is negligible (very very small)
- Constant, random, straight line motion
- Elastic collisions, meaning no energy is lost
- Pressure is low, temp is high
10
Q
Ideal Gas Law Formula
A
PV = nRT
Note: R = universal gas constant = 8.314 (kPa x L)/(mol x K)
