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Ideal Gas Law

21.43. 5.0. 1.0. 3.0. Ideal Gas Law. PV = nRT. no interactions. no volume. ideal gas. 24.88. SO 2. van der Waals. n 2 a. PV (L atm). P +. ( V – n b ). = nRT. V 2. a = interactive force. b = molecular diameter. 4.52. P (atm). gas. liquid. solid. Ideal gas.

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Ideal Gas Law

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  1. 21.43 5.0 1.0 3.0 Ideal Gas Law PV = nRT no interactions no volume ideal gas 24.88 SO2 van der Waals n2 a PV (L atm) P + ( V – nb) = nRT V2 a = interactive force b = molecular diameter 4.52 P (atm) gas liquid solid

  2. Ideal gas kinetic energy motion K.E. = ½ mv2 K.E.ave = 3/2 RT increase T increase energy Cv heat capacity = 3/2 R energy K

  3. Non-Ideal gas kinetic energy motion K.E. = = K.E.translation + K.E.rotation + K.E.vibration ½ mv2 He Rn degrees of freedom = 3n 3 translation H2 H2O

  4. Non-Ideal gas molar heat capacity heat required to change the temperature of 1 mole, 1K ideal gas 3/2 R K.E.translation K.E.translation + K.E.rotation + K.E.vibration non-ideal gas energy = heat capacity x T T = energy heat capacity  degrees of freedom heat capacity strength of Intermolecular Forces

  5. + + Non-Ideal gas kinetic energy motion K.E. = = K.E.translation + K.E.rotation + K.E.vibration ½ mv2 potential energy position electrostatic P.E. = Coulomb’s Law Q1Q2 charge 4 0 r distance P.E. 0 P.E.IMF related to a P.E.bond r

  6. Intermolecular Forces 2+ 2+ =  all types of forces van der Waals forces (2 kJ/mol) all types of molecules London Forces e- e- He e- e- - + - + e- b.p. instantaneous dipole He 2 -269 small short lived short distance Ne 10 -246 polarizibility strength increases Ar 18 -186 36 -152 Kr 54 -107 Xe size shape Rn 86 -62

  7. Intermolecular Forces =  all types of forces van der Waals forces (2 kJ/mol) all types of molecules London Forces C5H12 pentane neo-pentane b.p. = 36oC b.p. = - 9oC size shape

  8. Intermolecular Forces =  all types of forces van der Waals forces (2 kJ/mol) all types of molecules London Forces dipole - dipole (2 kJ/mol) polar molecules HCl dipole permanent charge separation + - - - - + + + + - C2H2Cl2 CO2 - + -

  9. Intermolecular Forces -N- =  all types of forces van der Waals forces (2 kJ/mol) all types of molecules London Forces dipole - dipole (2 kJ/mol) polar molecules hydrogen bonding donors and acceptors (20 kJ/mol) N-H + - + O-H + - -O- + - F-H F- + - high heat capacity ice less dense than water

  10. Intermolecular (Interionic) Forces Ion-ion metals and non-metals NaCl small distances large charges 250 kJ/mol m.p. 800oC NaCl + H2O Ion-dipole ions and polar molecules (aq) + Cl- (aq) Na+

  11. Intermolecular Forces HCl HBr b.p. = 206 K b.p. = 189 K stronger LDF 36 e- more polar 18 e- Solubility compatible IMF “likes dissolve likes”

  12. Surface Tension water on wax imbalance in IMF minimize surface  IMF surface tension cohesion adhesion glass is Si and O H-bond to water capillary action

  13. Viscosity Ns/m2  IMF fluid’s resistance to flow 9.7 x 10-4 CCl4 1.0 x 10-3 water 1.49 glycerol decreases with temperature

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