Ideal Gases Flashcards
Explain the kinetic theory of gases
- Gases are made up of small particles separated by large distances, therefore most of the volume occupied by a gas is empty space.
- Gaseous particles are always moving in straight lines, but random locations.
- gaseous particles undergo elastic collisions with each other and the walls of the container. No kinetic energy is lost.
- Gaseous particles exert no force of attraction on other gases.
State what is STP
Standard temperature (K) and Pressure (P)
What is an ideal gas?
A gas that is at STP and obeys the kinetic theory.
Does the following statement correspond to an ideal gas? : High temp and Low press. = forces of attraction are minimized
Yes, because it forces particles to have a high degree of separation.
Does the following statement correspond to an ideal gas? : Low temp and High press. = forces of attraction increase
No, because it exhibits its real behavior.
Explain the assumptions of the ideal gas model
- Molecules of gas are in constant motion
- Collisions between molecules are elastic (no transfer energy)
- The volume occupied by gas molecules is negligible compared to the volume of the container they occupy.
- There are no intermolecular forces between gas particles.
- The kinetic energy of molecules is directly proportional to K temperature.
At STP conditions what volume will have a gas?
22,4 L / mol or 22,7 L / mol
Operation to change from Volume (at STP) to moles and from moles to volume (at STP)
V to mol ( / 22,4L)
mol to V ( x 22,4L)
At STP there will be X number of molecules or atoms
6,02x10e23
Explain Boyle’s law
There is an inverse relationship between pressure and volume. If pressure increases volume decreases. If pressure decreases volume increases.
V1p1 = V2p2
Explain Charle’s law
For a fixed mass of a gas at a constant pressure the volume of the gas is directly proportional to the absolute temperature in K.
V1/T1 = V2/T2
Combined gas law:
8,31 J/ K mol or 0,0821 L atm/K mol
