ideal gases Flashcards
how to describe the motion of the smoke particles?
the visible smoke particles move with a random & jittery motion
what conclusions can we make about the motion of the invisible air particles?
- very fast moving (lots of momentum)
- collide with smoke particles- making them move randomly
explain the interaction between the invisible air particles & the visible smoke particles which causes the motion of the smoke particles
- fast moving invisible air molecules collide with visible smoke particles
- air particles transfer energy & momentum to the smoke particles, causing them to move randomly & jittery
molecules in a gas having a random motion and exerting a force means what for the pressure?
exert a force- hence pressure on the walls of the container
what does the temperature of the gas affect?
the speed of the gas molecules
what does higher temperature lead to?
faster moving molecules
what happens to the pressure if the volume doubles?
double volume : half pressure
what causes pressure from a gas on the side of a container?
- gas particles collide with wall of container
- particle changes direction & momentum as it rebounds
- particle exerts force on wall- wall exerts equal/ opposite force on particle
- pressure = force/area
if pressure on the sides of the container increases, what are the 2 reasons for this answer?
- particles hit with more force
- particles hit more frequently
air particles cannot be seen even with the highest power microscope- what does this tell us about the size of an air particle in comparison to the size of a smoke speck?
- air particles are much smaller than smoke particles
- to have more momentum to move the heavier smoke particles, air particles must be moving very quickly
why does the smell of deodorant diffuse across a room when only sprayed on one side?
- invisible fast moving air particles collide with the heavier deodorant particles, moving them in a random motion- making them diffuse into the room
what are the 4 ideal gas variables?
- pressure
- volume
- temperature
- the mass of gas
what do you need to fix when investigating pressure & volume?
fix temperature & mass
what is the relationship between pressure and volume?
pressure is inversely proportional to volume
what happens to the pressure if you double the volume?
- double volume
- half pressure
what is Boyle’s law?
- for a fixed mass of gas at a constant temperature- P1 x V1 = P2 x V2
- if volume doubles- pressure halves
- if pressure doubles- volume halves
what causes pressure in a gas?
- gas particles collide with the walls of the container
- particle changes direction & momentum as it rebounds
- particle exerts force on wall- wall exerts equal/ opposite force on the particles
- pressure = force/ area
P1 x V1 = P2 x V2 is only true when…
temperature & mass are constant
what happens to pressure if temperature increases, but volume & mass are fixed?
- increased pressure
- particles have more KE
- more frequent collisions
- harder (more forceful collisions)
what happens to the pressure if volume decreases but temperature & mass are fixed?
- pressure increases
- more frequent collisions
temperature always has to be in what measurement for all calculations in gases?
Kelvin
volume is inversely or directly proportional to temperature if pressure & mass are fixed?
directly proportional
how to convert degrees celsius to kelvin?
add 273
how to convert kelvin to degrees celsius?
subtract 273
