4 Gaseous State Flashcards
1
Q
Assumptions of the Kinetic Theory
A
- Gas particles are in constant random motion
- Gas particles have negligible volume/size compared to the volume of container
- Gas particles exert negligible intermolecular forces on one another
- Collisions between gas particles are perfectly elastic
- Average KE directly proportional to absolute temperature (in K)
2
Q
1 atm
A
101325 Pa
3
Q
Conversion from Kelvins to Celsius
A
T (K) = T (°C) + 273
4
Q
Ideal gas equation
A
pV=nRT
5
Q
Boyle’s Law
A
Constant temperature, volume of a fixed mass of gas is inversely proportional to its pressure (pV=constant)
6
Q
Charles’ Law
A
Constant pressure, volume of a fixed mass of gas is directly proportional to its absolute temperature in K (V/T=constant)
7
Q
Avogadro’s Law
A
Constant temperature and pressure, volume of a gas is directly proportional to the number of moles of gas (V/n=constant)
8
Q
Dalton’s Law of Partial Pressure
A
Total pressure of a mixture of non-reacting gases equals to the sum of the partial pressures exerted by the constituent gases.
9
Q
Deviation of ideal behaviour
A
- High pressure
- Large electron cloud/polar (stronger imf)
- Lower temperature
