ideal gas law pv = nrt pv (l atm) p (atm) 24.88 ideal gas so 2 1.03.0 5.0 4.52 21.43 no volume no...
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![Page 1: Ideal Gas Law PV = nRT PV (L atm) P (atm) 24.88 ideal gas SO 2 1.03.0 5.0 4.52 21.43 no volume no interactions van der Waals P + n 2 a V2V2 ( V – nb) =](https://reader038.vdocuments.net/reader038/viewer/2022103022/56649f505503460f94c72e4a/html5/thumbnails/1.jpg)
Ideal Gas Law PV = nRT
PV(L atm)
P (atm)
24.88 ideal gas
SO2
1.0 3.0 5.04.52
21.43
no volumeno interactions
van der Waals
P + n2 aV2
( V – nb) = nRT
a = interactive force
b = molecular diameter
gas liquid solid
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Ideal gas
kinetic energy motion
increase T
K.E. =
increase energy
½ mv2
K.E.ave = 3/2 RT
heat capacity
energyK
Cv = 3/2 R
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Non-Ideal gas
kinetic energy motion
K.E. = ½ mv2 = K.E.translation + K.E.vibration+ K.E.rotation
He
H2
degrees of freedom = 3n 3 translation
H2O
Rn
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Non-Ideal gas
molar heat capacity
ideal gas 3/2 R
heat required to change the temperatureof 1 mole, 1K
K.E.translation
non-ideal gas K.E.translation + K.E.rotation + K.E.vibration
energy = heat capacity x T T =
heat capacity
heat capacity degrees of freedom
energy
strength of Intermolecular Forces
![Page 5: Ideal Gas Law PV = nRT PV (L atm) P (atm) 24.88 ideal gas SO 2 1.03.0 5.0 4.52 21.43 no volume no interactions van der Waals P + n 2 a V2V2 ( V – nb) =](https://reader038.vdocuments.net/reader038/viewer/2022103022/56649f505503460f94c72e4a/html5/thumbnails/5.jpg)
Non-Ideal gas
kinetic energy motion
K.E. = ½ mv2 = K.E.translation + K.E.vibration+ K.E.rotation
electrostatic
P.E. = Coulomb’s Law Q1Q2
4 0 rchargedistance
potential energy position
P.E.
r
0
related to a
P.E.bond
P.E.IMF
++
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He
- +
small short lived
strength increases
size
HeNeArKrXeRn
21018365486
-269-246-186-152-107-62
e- b.p.
2+
e-
e-
2+
e-
e-
shape
van der Waals forces
London Forces
= all types of forces
(2 kJ/mol) all types of molecules
dipole - +
short distance
polarizibility
instantaneous
Intermolecular Forces
![Page 7: Ideal Gas Law PV = nRT PV (L atm) P (atm) 24.88 ideal gas SO 2 1.03.0 5.0 4.52 21.43 no volume no interactions van der Waals P + n 2 a V2V2 ( V – nb) =](https://reader038.vdocuments.net/reader038/viewer/2022103022/56649f505503460f94c72e4a/html5/thumbnails/7.jpg)
shape
pentaneneo-pentane
C5H12
b.p. = 36oC b.p. = - 9oC
size
van der Waals forces = all types of forces
London Forces (2 kJ/mol) all types of molecules
Intermolecular Forces
![Page 8: Ideal Gas Law PV = nRT PV (L atm) P (atm) 24.88 ideal gas SO 2 1.03.0 5.0 4.52 21.43 no volume no interactions van der Waals P + n 2 a V2V2 ( V – nb) =](https://reader038.vdocuments.net/reader038/viewer/2022103022/56649f505503460f94c72e4a/html5/thumbnails/8.jpg)
Intermolecular Forcesvan der Waals forces = all types of forces
dipole - dipole polar molecules
permanent charge separationHCl
London Forces (2 kJ/mol) all types of molecules
dipole
(2 kJ/mol)
-+
- -
+ ++ +
-
-
- -+
C2H2Cl2
CO2
![Page 9: Ideal Gas Law PV = nRT PV (L atm) P (atm) 24.88 ideal gas SO 2 1.03.0 5.0 4.52 21.43 no volume no interactions van der Waals P + n 2 a V2V2 ( V – nb) =](https://reader038.vdocuments.net/reader038/viewer/2022103022/56649f505503460f94c72e4a/html5/thumbnails/9.jpg)
Intermolecular Forcesvan der Waals forces = all types of forces
dipole - dipole polar molecules
London Forces (2 kJ/mol) all types of molecules
(2 kJ/mol)
hydrogen bonding (20 kJ/mol) donors and acceptorsN-HO-HF-H
+
+
+ F--O--N--
-
--
+
+
ice less dense than water
high heat capacity
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Intermolecular (Interionic) Forces
Ion-dipole ions and polar molecules
NaCl + H2O
Na+
Ion-ion metals and non-metalsNaCl
250 kJ/mol large charges small distancesm.p. 800oC
(aq) + Cl- (aq)
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Intermolecular Forces
HCl HBr
b.p. = 189 K b.p. = 206 K
18 e- 36 e-more polar stronger LDF
Solubility“likes dissolve likes” compatible IMF
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Surface Tension
water on waximbalance in IMF minimize surfacesurface tension IMF
glass is Si and O
H-bond to water capillary action
cohesion adhesion
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Viscosity
fluid’s resistance to flow IMF
CCl4
water
glycerol
9.7 x 10-4
Ns/m2
1.0 x 10-3
1.49
decreases with temperature