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ideal gases Flashcards

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1
Q

how to describe the motion of the smoke particles?

A

the visible smoke particles move with a random & jittery motion

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2
Q

what conclusions can we make about the motion of the invisible air particles?

A
  • very fast moving (lots of momentum)
  • collide with smoke particles- making them move randomly
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3
Q

explain the interaction between the invisible air particles & the visible smoke particles which causes the motion of the smoke particles

A
  • 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
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4
Q

molecules in a gas having a random motion and exerting a force means what for the pressure?

A

exert a force- hence pressure on the walls of the container

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5
Q

what does the temperature of the gas affect?

A

the speed of the gas molecules

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6
Q

what does higher temperature lead to?

A

faster moving molecules

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7
Q

what happens to the pressure if the volume doubles?

A

double volume : half pressure

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8
Q

what causes pressure from a gas on the side of a container?

A
  • 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
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9
Q

if pressure on the sides of the container increases, what are the 2 reasons for this answer?

A
  • particles hit with more force
  • particles hit more frequently
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10
Q

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?

A
  • 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
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11
Q

why does the smell of deodorant diffuse across a room when only sprayed on one side?

A
  • invisible fast moving air particles collide with the heavier deodorant particles, moving them in a random motion- making them diffuse into the room
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12
Q

what are the 4 ideal gas variables?

A
  • pressure
  • volume
  • temperature
  • the mass of gas
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13
Q

what do you need to fix when investigating pressure & volume?

A

fix temperature & mass

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14
Q

what is the relationship between pressure and volume?

A

pressure is inversely proportional to volume

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15
Q

what happens to the pressure if you double the volume?

A
  • double volume
  • half pressure
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16
Q

what is Boyle’s law?

A
  • 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
17
Q

what causes pressure in a gas?

A
  • 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
18
Q

P1 x V1 = P2 x V2 is only true when…

A

temperature & mass are constant

19
Q

what happens to pressure if temperature increases, but volume & mass are fixed?

A
  • increased pressure
  • particles have more KE
  • more frequent collisions
  • harder (more forceful collisions)
20
Q

what happens to the pressure if volume decreases but temperature & mass are fixed?

A
  • pressure increases
  • more frequent collisions
21
Q

temperature always has to be in what measurement for all calculations in gases?

A

Kelvin

22
Q

volume is inversely or directly proportional to temperature if pressure & mass are fixed?

A

directly proportional

23
Q

how to convert degrees celsius to kelvin?

A

add 273

24
Q

how to convert kelvin to degrees celsius?

A

subtract 273

25
Q

what is the relationship between pressure & temperature?

A
  • pressure is directly proportional to temperature
  • for a fixed mass & volume
26
Q

what is the formula linking pressure & temperature together?

A

P1/T1=P2/T2

27
Q

what is the relationship between pressure & temperature?

A

they are directly proportional

28
Q

why is there an absolute zero of temperature which is -273 degrees celsius (0K)?

A

the particles completely stop moving

29
Q

increasing the temperature of a gas results in an increase of what variable about the molecule?

A

an increase of kinetic energy

30
Q

the kelvin temperature of a gas is proportional to what?

A

the KE of its molecules

31
Q

as kelvin temperature increases what else about the gas increases?

A

the speed of the molecules

32
Q

what is the formula for pressure in a liquid?

A

hpg- depth x density x gravity

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