gas laws Flashcards

1
Q

kinetic molecular theory (ideal gas laws)

A

a theory used to explain / describe the usual behavior of gases
- theory describes the relationship among:
- pressure
- volume
- temp
- velocity
- frequency of collisions

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2
Q

ideal gas laws (kmt)

A
  • gases contain particles that are in constant, random, and “straight-line” motion
  • gas particles collide with each other and with the walls of the container
    • results in a transfer of energy
  • gas particles are separated by great distances
    • no definite volume or shape
  • gas particles DO NOT attract each other
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3
Q

ideal vs real gas laws

A

ideal : kmt
- gases are most ideal at low pressure and high temp
- hydrogen and helium are always ideal gases (low density)

real:
- gas particles DO attract each other
- gas particles DO occupy volume
- gases are most REAL at high pressure and low temp

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4
Q

avogadro’s hypothesis

A

if two gases are at the same exact temp and pressure…
- the volume that the gases occupy are the same AND the # moles (# molecules) are also the same
- if gases happen to be at STP, every 1 moles of gas would occupy 22.4 L

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5
Q

boyle’s law

A

P1V1 = P2V2

at constant temp:
- as pressure increases on a gas, volume will decrease
- pressure and volume are inversely proportional

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6
Q

charles’ law

A

V1 / T1 = V2 / T2

at constant pressure:
- volume is directly proportional to its change in temp
temp must be measured in KELVIN

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7
Q

lussac’s law

A

P1 / T1 = P2 / T2

at constant volume:
- as temp increases, pressure exerted by the gas will increase
- directly proportional

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