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Understanding Gas Laws: Boyle’s, Charles’, and Avogadro’s Theories Explained

This comprehensive overview of gas laws delves into Boyle’s Law (pressure-volume relationship), Charles’ Law (volume-temperature relationship), and Avogadro’s Law (volume-mole relationship). Additionally, it explores the Ideal Gas Equation, PV = nRT, and its applications including density calculations and Dalton’s Law of partial pressures. The Kinetic Molecular Theory describes gas particle behavior and the concepts of effusion and diffusion, providing insights into real gas behavior and deviations from ideal gas laws at varying pressures and temperatures.

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Understanding Gas Laws: Boyle’s, Charles’, and Avogadro’s Theories Explained

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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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