CHM 2046C Lecture Notes - Lecture 6: Spontaneous Process, Joule, Thermodynamics

36 views5 pages
20 Apr 2016
School
Department
Course
Professor

Document Summary

Lecture 6 notes: first law of thermodynamics: energy cannot be created or destroyed, -it can be transferred from one place to another, -or, the total energy of the universe cannot change. Deuniverse = 0 = desystem + desurroundings. Surroundings = everything else: enthalpy, h, related to the internal energy, e (e + pv = h) Dh = qp; generally kj/mol: if products are more stable than reactants, energy (heat) released, hence Dh = positive (+ve) or negative (-ve): if reactants are more stable than products, energy (heat) absorbed, hence K = boltzmann constant (r/na) = 1. 38 10-23 j/k. W is the number of energetically equivalent ways (microstates) to arrange the components; unitless: changes in entropy, ds. Entropy change is favorable when the result is a more random system: ds is positive (ds > 0) Some changes that increase the entropy are:

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related Documents

Related Questions