Gas Laws Quiz - Chemistry Sophomore year

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21 Terms

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KINETIC MOLECULAR THEORY

KINETIC MOLECULAR THEORY

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there are _ Posutlates

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The postulates are:

  1. gas particles are in constant motion

  2. the combined volume of the paritcles of gas sample is negative compared to the volume of a container

  3. there are no attractive forces between the particles of a gas sample (so we assume)

  4. collisions between the gas particles ate completely elastic (meaning no energy is used)

  5. the average kinetic energy of gas particles in a sample is directly proportional to the kelvin temperature

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Pressure =

force applied over a specific area

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Why do gas particles exert pressure?

in constant motion, the particles collide with the walls of the container

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How can we increase pressure?

  1. increase temperature

  2. decrease volume of the container

  3. add more gas particles

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Units for pressure

atm = atmosphere (of pressure)

Kpa = kiloPascal

mmHg = millimeter of Mercury (torr)

psi = pounds per square inch (tire pressure)

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STP VALUES

1 atm = 101.3 kPa = 760 mmHg(torr)

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How many atm is 252 kPa?

252 kPa x 1 atm/101.3 kPa = 2.49 atm

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BOYLE’S LAW

BOYLE’S LAW

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Boyle’s law =

the relationship between pressure and volume

inversely proportional relationship

Equation = P1V1 = P2V2

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example

P1V1 = P2V2

(103.1kPa)(1.00L) = P2 (0.35L)

divide both sides of 0.35L

P2 = 295 kPa

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CHARLES’S LAW

relationship between temperature and volume

directly proportional relationship

Equation = V1/T1 = V2/T2

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Temperature Must be in..

Kelvin (because it does not have any negative numbers)

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To convert celsius to Kelvin…

add 273 to the celsius

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Gay-Lussac’s Law

relationship between pressure and temperature

directly proportional relationship

Equation = P1/T1 = P2/T2

Temp must be in kelvin

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Combined Gas Law

looks at relationship between pressure,volume, and temperature when all 3 values are changing

Equation = P1V1/T1 = P2V2/T2

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STP =

1 atm, O degrees Celsius, 273 kPa

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The Ideal Gas Law

no change in conditions

Equation = PV = nRT

R = gas law constant

n = number of moles

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IDEAL GAS LAW CONSTANT

0.08206 L x atm/mol x K

8.314 L x kPa/mol x K

62.36 L x torr/mol x K

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To calculate the number of moles to grams it is…

number of moles (n) x molar mass/1 mole