CHE 111 Lecture Notes - Lecture 21: Exothermic Process, Isolated System, Thermodynamics

• School: Quinnipiac University
• Department: Chemistry
• Course: CHE 111
• Professor: O'Keefe

Document Summary

1st law: usystem + usurroundings = 0. 2nd law: process spontaneous suniverse > 0. S > 0 has to suniversal (open + closed) Doesn"t matter how we go from initial to final state. U = q + w q = heat w = work w = force x distance. Area = a w = force x distance x a/a w = f/a x da height x area = volume w = pressure x volume. H = u + p v w is negative from system"s point of view for constant pressure process. H = q - p v + p v = qsystem. G (gibbs free energy) = h - ts. G < 0 rxn spontaneous in forward direction. G > 0 rxn spontaneous in reverse direction. An exothermic rxn h= ---, g < 0. If s is negative, then g < 0 when | h| is greater than |t s|