Download KMT and Ideal Gas Notes 2016

Avogadro and Ideal Gases 2016.notebook
November 03, 2016
Kinetic Molecular Theory of Gases
Aim: What is an ideal gas? How can a real gas behave
most like an ideal gas?
Oct 17­11:05 AM
Marble Activity
Oct 29­8:05 AM
1
Avogadro and Ideal Gases 2016.notebook
November 03, 2016
Properties of an Ideal Gas
1. Ideal gas particles are so small as compared with the distance
separating them that the volume of the particle is considered
negligible (zero).
2. Ideal gas particles travel in constant, random, straight-line
motion. (SAME AS REAL GASES)
3. Ideal gases have no intermolecular forces (attraction) between
particles.
4. The collisions of the particles are elastic (complete transfer of
energy, no kinetic energy is lost as a different form)
5. Equal volumes of any gas will have an equal number of particles.
Oct 17­11:05 AM
Ideal Gases Do Not Exist
Real gases DO NOT behave like an ideal gas because:
• Real gases HAVE intermolecular forces b/w particles.
• Real gas particles HAVE volume.
• Real gases LOSE energy upon colliding (inelastic collision)
The only similarity between a real and ideal gas is that both move in
constant, random, straight-line motion.
Oct 17­11:05 AM
2
Avogadro and Ideal Gases 2016.notebook
November 03, 2016
Behaving like an Ideal Gas
How can we use temperature and pressure to allow for weak attractions and far distance between particles?
emperature
igh
ases
deal
ow
ressure
Real gases behave most like ideal gases when:
-the attractions between molecules are weak
-the molecules are far apart from each other.
Real gases can behave ideally under certain conditions:
P
L
I
G
H
T
Oct 17­11:05 AM
Real gases that behave the most ideal.
• H2 (hydrogen) & He (Helium) behave most like an ideal gas
compared to other gaseous elements.
• This is because the smallest gases have the weakest
attractions and most space between particles.
• This allows them to behave most ideal.
Oct 17­11:05 AM
3
Avogadro and Ideal Gases 2016.notebook
November 03, 2016
Avogadro‛s and Gases
Avogadro was a scientist who discovered
the MOLE.
A mole is a way of measuring large
quantities of particles.
1 mole= 22.4 Liters= 6.02 x 1023 particles.
• Avodagro's Theory: equal volumes of any gas
that are equal always contain an equal number of
particles because the number of moles is equal.
Nov 18­1:55 PM
4