Home > Uncategorized > Thermodynamics and Kinetics Lecture 23 Notes

Thermodynamics and Kinetics Lecture 23 Notes

Today’s lecture is 51 minutes long. This class is shared among two teachers.

Pa = Xa Pa*

Very small amounts of solute require Henry’s Law. Raolt’s law is for situations when there is alot of solute. Solvent molecules need to see molecules other than themselves.

A and B in a dilute, non ideal solutions. At 50C, Pa* = 0.67 bar, Pb*=1.7 bar. Thus B is more volatile. Xa = 0.9, Xb = 0.1, Pt = 0.9 bar. A is the solvent, B is the solute. We can use Hank’s law for b, Raolt for A.

Pt = Pa + Pb = xa Pa* + Xb Kb (Henry’s Law)
Kb = Pb/Xb

Azeotropes cannot be seperated by fractional distillation.

Colligative properties: vapor pressure depression, BP elevation, MP depression, osmotic pressure.

Molality = moles solute/kg solvent = moles/weight

Molarity = moles/Liter

dTv = Kb Mb

d (dG/T)/dT = -dH/T
The Gibbs HelmHoltz Equation

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Intermolecular Forces: ionic, hydrogen bonding, dipole dipole, VdW

1st Law dU=dW + dQ
2nd Law dS = dq rev/T
3rd law, oK – S=O

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