GEN CHEM Ch. 6 Gases

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Last updated 4:44 AM on 5/27/26
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16 Terms

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Ideal Gas Law (Kinetic-Molecular Theory of Gases)

  1. Particles in a gas are in constant, random motion

  2. The combined volume of particles is negligible

  3. Particles exert no force on one another

  4. Gas molecule collisions are entirely elastic, indicating no intermolecular forces

  5. All gases have the same average kinetic energy at a given temperature KEavg∝ (T + 273 K)

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Assuming the same number of moles, in which of the conditions would a gas behave most ideally?

Kinetic-Molecular Theory of Gases – gases behave most ideally at low pressures and high temperatures.

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effusion

r1 / r2 = sqrt(M2 / M1)

confined gas escapting through a small hole

  • gas > liquild > solid

  • gas w/ lowest molar mass effuses faster

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diffusion

molecules move from [high] → [low]

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gas laws: Boyle, Charles, Avogadro, Gay-Lussac, combined gas

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Boyle’s Law

P1V1 = P2V2

pressure (atm) and volume (L) are inversely proportional under constant temperature and moles.

<p>P<sub>1</sub>V<sub>1</sub> = P<sub>2</sub>V<sub>2</sub></p><p>pressure (atm) and volume (L) are inversely proportional under constant temperature and moles.</p>
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Charles’s Law

V𝟣 / T𝟣 = V𝟤 / T𝟤

volume (L) and temperature (K) are directly proportional under constant pressure and moles

<p>V<sub>𝟣</sub> / T<sub>𝟣</sub> = V<sub>𝟤</sub> / T<sub>𝟤</sub></p><p>volume (L) and temperature (K) are directly proportional under constant pressure and moles</p>
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Avogadro’s Law

V𝟣 / n𝟣 = V𝟤 / n𝟤

volume (L) and moles (mol) are directly proportional under constant pressure and temperature

<p>V<sub>𝟣</sub> / n<sub>𝟣</sub> = V<sub>𝟤</sub> / n<sub>𝟤</sub></p><p>volume (L) and moles (mol) are directly proportional under constant pressure and temperature</p>
9
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Gay-Lussac’s Law

P𝟣 / T𝟣 = P𝟤 / T𝟤

pressure (atm) and temperature (K) are directly proportional under constant volume and moles

<p>P<sub>𝟣</sub> / T<sub>𝟣</sub> = P<sub>𝟤</sub> / T<sub>𝟤</sub></p><p>pressure (atm) and temperature (K) are directly proportional under constant volume and moles</p>
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Combined Gas Law

P𝟣V𝟣 / n𝟣T𝟣 = P𝟤V𝟤 / n𝟤T𝟤

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partial pressure involving mole fractions

P1 = X1Ptotal

X1 = mol1 / moltotal

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relationship between pressure (P), force (F), and area (A)

P = F / A

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Ideal Gas Law

PV = nRT (use when question mentions ideal)

P = pressure V = volume n = moles R = ideal gas constant T = temperature

R = 0.0821 L*atm/mol*k or 8.314 L*kPa/mol*K

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STP Conditions

  • 273 K

  • 1 atm

  • 22.4 L in 1 mole

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gas density

ρ = m / V = PM / RT

ρ = density m = mass V = volume P = pressure M = molar mass R = ideal gas constant T = temperature

R = 0.0821 L*atm/mol*k or 8.314 L*kPa/mol*K

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1 atm conversions

1 atm = 760 mmHg = 760 torr = 101.325 kPa = 101,325 Pa