Week 2 Day 3 Gas laws
No description yet. This curated deck is ready for daily study.
Card preview (14)
Which gas law relates volume and pressure? (Temp is constant)
Boyle’s Law increased pressure → decreased volume inverse relationship “If you compress something, it gets smaller!”
According to Charles Law, if you heat something up…..
it expands! increased temperature → increased volume (pressure constant) proportional relationship
According to Gay-Lussac’s law, if you heat something, what happens to the pressure?
the pressure increases! increased temperature → increased pressure
What does Avogadro’s law tell us about equal volumes of gases at the same temperature and pressure, in regards to # of particles?
equal volumes of different gases have the same # of particles
According to Avogadro’s Law, if we add more particles, what happens to volume?
volume gets bigger! increased particles → increased volume
Measure of the degree of saturation of H20 in the air
relative humidity
Dew point
point at which water condenses because warm air holds more water than cool air, so as air cools, it is possible for the amount of water in the air to exceed solubility → condensation
Name the 4 assumptions of the Kinetic Molecular Theory of Gases
1. gas molecules are small compared to the volume of the gas, so we can ignore the size of the molecule 2. gas molecules are in constant, random motion 3. gas molecules show a range of kinetic energies, but the average depends on the temperature 4. gas molecules are not attracted or repulsed from each other, so all collisions are elastic
Graham’s Law of Effusion (or Diffusion)
smaller particles move faster! and heating them up also moves them faster
Under what 2 circumstances do real gases not behave like ideal gases?
very high pressure or very low temperature
Which 2 assumptions of ideal gases hold true for real gases?
2 and 3 • gas molecules are in constant, random motion • gas molecules show a range of kinetic energies, but the average depends on the temperature.
For ideal gases, we assume that (1) gas molecules are small compared to the volume of the gas, so we can ignore the size of the molecule. Why is this not entirely true?
we cannot completely ignore the size of the particles, especially as concentration is increased at high pressure
For ideal gases, we assume that (4) gas molecules are not attracted or repulsed from each other, so all collisions are elastic. Why is this not entirely true?
gas particles are very weakly attracted, so if the particles move slowly enough, at very low temperatures, this attraction matters
True or False: Real gases approach ideal gas behavior as pressure increases and temperature decreases.
False Real gases approach ideal gas behavior as pressure decreases and temperature increases.