Chem 162-2011 Lecture 18, 17.5-17.6

Chem 162-2011 Lecture 18, 17.5-17.6 - CHEMISTRY 162-2011...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: CHEMISTRY 162-2011 LECTURE 18 Ed Tavss, PhD ANNOUNCEMENTS E-MAIL ATTENDANCE Sign in EXAMS RECITATION QUIZ Friday: H&P: 20.7-20.9; 17.1-17.3 (My lectures 16 & 17) MISCELLANEOUS You are invited to attend our Spring open advising sessions for chemistry majors and minors. Non-majors with questions pertaining to chemistry courses are also welcome. These sessions will be held in Doolittle 108 (Busch) on weekdays April 1 through April 12, from 4 pm until 5:30 pm. This schedule covers the Spring registration days for Fall 2011 classes. John Taylor, Vice Chair of the Undergraduate Program in Chemistry Chem 162-2011 Lecture 1 PLAN FOR TODAY CHAPTER 17 - SPONTANEITY, ENTROPY AND FREE ENERGY 17.5 Standard free energy change, G o 17.6 Free energy change and equilibrium If there is time at the end Ill review optical isomers. I believe that optical isomers is the most difficult part of Coordination Compound isomers. Chem 162-2011 Lecture 2 CHAPTER 16- SPONTANEITY, ENTROPY AND FREE ENERGY First law of thermodynamics: Energy can neither be created nor destroyed. Second law of thermodynamics: The entropy of the universe always increases in a spontaneous process. Third law of thermodynamics: The entropy of a perfectly ordered crystalline substance at 0 K is zero. Entropy describes the number of arrangements (positions and/or energy levels) available to a system. Entropy is (officially called chaos, disorder, randomness) positional freedom, or positional availability, or disorder, or being unconfined positionally or escape from positional confinement or freedom from positional confinement G o = n p G o f(products)- n r G o f(reactants) H o = n p H o f(products)- n r H o f(reactants) S o system = n p S o products- n r S o reactants S system = n p S products- n r S reactants (used for S system anytime ) S system = H system /T (used for S system only when at equilibrium) S surr = H surr /T = -H system /T (used for S surr anytime) S univ = S sys + S surr Four ways to find G o : (1) G o = H o- TS o (or G = H - TS) At equilibrium G = 0 0 = (H - TS) S system = H system /T Troutons rule: At normal B.P., S vaprization 87J mol-1 K-1 (2) G o = n p G o f(products)- n r G o f(reactants) (3) G T o = G 1 o + G 2 o (i.e., Coupling Reactions [i.e., Hesss law]) (4) G o = -RT ln(K) G = G o + RT ln(Q) (Q can be any pressure or concentration) w max = G ln(K 2 /K 1 ) = (H o /R)((1/T 1 ) (1/T 2 )) Chem 162-2011 Lecture 3 Concepts: Reaction: A + 2B 3C + D G = H - TS Spontaneous process: a reaction that goes forward without any outside intervention; a reaction that goes to the right....
View Full Document

This document was uploaded on 11/02/2011 for the course GEN CHEM 162 at Rutgers.

Page1 / 16

Chem 162-2011 Lecture 18, 17.5-17.6 - CHEMISTRY 162-2011...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online