CHEM 123 Lecture Notes - Lecture 7: Endergonic Reaction, Exergonic Reaction, Exergonic Process

• School: UBC
• Department: Chemistry
• Course: CHEM 123
• Professor: Erin Lindenberg

Document Summary

3rd law reference pt. of s (t = 0k, Change in s = 0 crystal: entropy, gibbs free e. S= k*lnw = 0 lnw = 0 e^(lnw) = e^0. If it was converted from perfect crystalline form. Absolute s of 1mol of substance in its standard state (units j/kmol) Note: need change in suniv to tell if spontaneous. Greater increase in change in ssurr than decrease in change in sreaction. Use gibbs free e (look at system only) ds = dqrev/t. Gibbs free e of the system (j/kj) definition. Change in g = change in h - t*change in. Change in ssys + change in s surr. Change in s surr = -qrev, sys/t. Change in suni = change in ssys - qrevsys/t. *h is the e/q released by bond breaking/forming (ie. -h is preferred since reactants want to be in a lower e state 1st law?) Exergonic (lose e not q from initial to final)