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Chemistry > Gas Laws > Flashcards

Gas Laws Flashcards

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1
Q

Kinetic Model Theory (KMT)

A

Explains matter (mostly gasses) as a simple model

  1. Matter consists of tiny particles
  2. Gasses have volume as a group
  3. Gasses have perfect elastic collisions (gas does not lose energy on collision and instead goes back to where it came from).
  4. There are no attraction or repulsion forces for gasses.
  5. Average kinetic energy = average temp. (k)
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2
Q

Temperature Symbol/Units

A

Symbol- T
Units - Kelvin, K

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3
Q

Pressure Symbol/Units

A

Symbol - P
Units - Atmospheric pressure, atm, Millimeters of Mercury, mmHg, Kilopascal, kPa

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4
Q

Volume Symbol/Units

A

Symbol - V
Units - Any form of liters, mL, L

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5
Q

Moles Symbol/Units

A

Symbol - n
Units - Moles, mol

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6
Q

Standard Atmospheric Pressure (STP)

A

Measured at sea level
1 atm
101.3 kPa
760 mmHg (Torr)

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7
Q

Standard Temperature

A

273 K (0 C)
Celsius –> K is C+273=K

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8
Q

Boyle’s Law

A

Relates pressure and volume
Temp. is held constant
Pressure and volume have an INVERSE relationship, when temperature is held constant

P1 V1 = P2 V2

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9
Q

Charles’ Law

A

Volume and temperature
Pressure is held constant
Volume and temperature have a DIRECT relationship, when pressure is held constant

V1/T1 = V2/T2

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10
Q

Gay - Lussac’s Law

A

Pressure and temperature
Volume is held constant
Pressure and temperature have a DIRECT relationship, when volume is held constant

P1/T1 = P2/T2

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11
Q

Combined Gas Law

A

P1 V1/T1 = P2 V2/T2

Must convert C to kelvin

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12
Q

Barometer

A

Measures atmospheric pressure

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13
Q

Manometers

A

Measures gas pressure

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14
Q

Gas Pressure

A

Patm + height of mercury (mmHg)

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15
Q

Dalton’s Law of Partial Pressure

A

Ptotal = P1 + P2 + P3…..etc

All pressures have the same units

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16
Q

Graham’s Law

A

Diffusion - Gas spreads out from high to low concentration
Ex. Perfume is sprayed on one side of a room and can be smelt on the other side

Effusion - Gas passes through small openings
Ex. Air slips out of balloons through small holes

Both depend on temp. of gas and molar mass of the gas
High temp. = fast gas
Small molar mass = fast gass
Fastest gas goes no top (of left side of formula)

Speed of gas A/ Speed of gas B = (sq. root) Molar mass B/Molar mass A

Chemistry (13 decks)

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