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Gases

Gases. Chapter 10. 10.3 Gas Laws. Boyle’s Law: P vs. V Charles’ Law: V vs. T Avogadro’s Law: V vs. n. Pressure. volume. volume. volume. moles. temperature. 10.4 Ideal Gas Equation. PV = nRT R = 0.0821 L • atm • mol -1 • K -1 If nR = constant then P 1 V 1 /T 1 = P 2 V 2 /T 2.

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Gases

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  1. Gases Chapter 10

  2. 10.3 Gas Laws • Boyle’s Law: P vs. V • Charles’ Law: V vs. T • Avogadro’s Law: V vs. n Pressure volume volume volume moles temperature

  3. 10.4 Ideal Gas Equation • PV = nRT R = 0.0821 L•atm•mol-1•K-1 • If nR = constant • then P1V1/T1 = P2V2/T2

  4. 10.5 Further Applications • Density = g/L • Density = g/mol • mol/L (=g/L) • Density = molar mass • n/V (=g/L) • Finally… molar mass = density•(RT/P)

  5. 10.6 Mixtures & Partial Pressure • Dalton’s Law: Ptot = P1 + P2 + P3 + … • Mole fraction: X1 = n1/nt = P1/Pt • Collecting gas over water: Ptot = Pgas + PH2O

  6. 10.7 Kinetic Molecular Theory • Gas particles are in constant, random, rapid, straight-line motion • Volume of a gas is mostly empty space • Attractions between particles are negligible • Collisions between particles are elastic (average k.e. = constant) • Average kinetic energy is directly proportional to absolute temperature

  7. 10.8 Effusion/Diffusion • Effusion: escape to an evacuated space through a small hole • Diffusion: mix/spread • Temperature determines K.E. • KE = 1/2mu2 • Lighter gases travel faster u = √(3RT/mm) • Graham’s Law: r1/r2 = √(mm2/mm1) • Mean free path: distance traveled before a collision

  8. 10.9 Real Gases • Deviation from ideal behavior is minimal: • below 10atm – at high pressures molecules take up space and attractions are measurable • Above boiling point for any gas – low temperatures causes an increase in effect of attractions • Van der Waals effect: • a & b are different for every gas nRT n2a V - nb V2 Correction for molecular volume Correction for attractions

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