S1.5 Ideal gases Flashcards
1
Q
ideal gas
A
- elastic collisions, no kinetic energy lost
- no intermolecular forces, pressure is less than expected by the ideal gas equation
- molecules have hardly any volume (negligible)
- gas temperature is directly proportional to the average kinetic energy of molecules
- molecules are very small compared to container size (small volume)
2
Q
kinetic theory of gases
A
molecules in gases are constantly moving
3
Q
real gases
A
- deviate from ideal gases, especially at low temperature and high pressure
- finite volume
- inelastic collisions
- intermolecular collisions
4
Q
when is the molar volume of an ideal gas constant
A
at a specific temperature and pressure
5
Q
Boyle’s law
A
As pressure increases, volume decreases
V∝1P
6
Q
Charles’ law
A
Increase the temperature, gas volume increases
More kinetic energy in particles, more frequent collisions
V∝T
7
Q
Gay-Lussac’s Law
A
Hotter gas, higher pressure
More kinetic energy, particles move faster, more frequency collisions with wall
P∝T
8
Q
ideal gas equation
A
PV = nRT
shows the relationship between pressure, volume, temperature and amount of ideal gas
9
Q
combined gas law
A
(P1V1)/T1 = (P2V2)/T2
shows the relationship between pressure, volume, temperature and amount of ideal gas
