Properties Of Gases Flashcards
Converting Celsius to Kelvin
+ 273
- 273 C / 0K or absolute zero
Considered to be the lowest temperature
Gas occupies 0 volume if it could be cooled without being a liquid or solid
Presure
Force (newton) / area (m*2)
Normal/standard atomospheric pressure
1 x 105 Pa or 100kPa
Gas
A sunstance that has no well-defined boundaries but diffuses rapidly to fill any container in which it is placed
Boyle’s Law definition
At constant temperature, the volume of a fix mass of gas is inversely proportional to its pressure
pV = k
(As the pressure increases the volume decreases)
Charles’ Law
At constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature measured on the Kelvin Scale V/ T = k
(When temperature increases preasure increases but in order to keep pressure constant we increase the volume)
Combined Gas Law
P1V1/T1 = P2V2/T2
Gay Lussac’s Las of Combing Volumes
In a reaction between gases, the volumes of the reacting gases and the volumes of any gaseous products are in the ratio of small whole numbers provided the volumes are measured at the same temperature and pressure
(2 volumes + 1 volume = 2 volumes)
Avogadro’s Law
Equal volumes of gases contain equal numbers of molecules under the same conditions of temperature and pressure
(1 molecule + 1 molecule = 2 molecules)
Density
Mass/volume
Assumptions of kinetic theory of gases
Particles in gases are in continuous rapid motion colliding with the container and each other
No attractive or repulsive forces between molecules
Gas molecules are so small + separated the actual volume negligible compared go to the space it occupies
When molecules collide - no loss of kinetic energy (perfectly elastic)
Average kinetic energy of a molecule in a gas is proportional to temperature in Kelvin
Limitations of Kinetic Theory of Gases
All gases have at least a small attraction or repulsive forces between molecules in a gas
Volume of a gas is not negligible since the pressure increases
Ideal gases don’t exist, similar conditions are
Widely spaced at low pressure
High temperature and pressure forces of attraction and repulsion don’t work as well
Ideal gas
One that perfectly obeys all the assumptions of the kinetic theory of gases under all conditions of temperature and pressure
Real gas
Differ from ideal gases because the forces of attraction and repulsion do exist between the molecules and the volume of the molecules is not negligible
