Home > Uncategorized > Thermodynamics and Kinetics Lecture 13 Notes: Gibbs Free Energy

Thermodynamics and Kinetics Lecture 13 Notes: Gibbs Free Energy

Overview
Today’s lecture is 50 minutes long.

Details
The direction of spontaneous change is related to G.
2nd law dS>dq/T for spontaneous change
1st law dU = dq + dW

The basic thermodynamic quantities are H, A, G and U. There are the fundamental equations. Everything is in terms of state variables. Path doesn’t matter.

d2A/dVdT = d/dv (dA/dT)

PV = nRT
(dP/dT)v = nR/V (dS/dV)T

VdW gas
(P-A/V2)(V-b2)=nRT

We wish to minimize energy and maximize entropy.

A = A(T,V) dA=-SdT -pdV
H = H (S,P) dH=TdS + VdP
U=U(S,V) dU=TdS-pdV
G=G(T,P) dG=-sdT + VdP

Review:

Aromatic: planar, cyclic, Huckels Rule – 4n+2 electrons

Fibrous – sclera, cornea

Sensory – retina

Vascular – choroid, iris, pupil, ciliary body

Kingdoms – monera, protista, fungi, plant, animal

HSbF6 pKa = 25

Electrophiles are positive, nucleophiles are negative

EDTA is a tetraprotic acid.

C-C=O-C Ketone

Ketones containing alkene and alkyne units are often called unsaturated ketones.

Ph2CO Benzophenone

Sunflower 8 benzenes fused together

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