final_exam_rev

final_exam_rev - MIT OpenCourseWare http:/ocw.mit.edu 5.60...

Info iconThis preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
MIT OpenCourseWare http://ocw.mit.edu 5.60 Thermodynamics & Kinetics Spring 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms .
Background image of page 1

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

View Full DocumentRight Arrow Icon
5.60 Final Exam Review 1. Phase Equilibria- 2 components a. Drawing P-x,y and T-x,y diagrams 2. Ideal and Non Ideal Solutions a. Raoult’s Law, Henry’s Law, Dalton’s Law i. Dalton’s Law: p A = y A p ii. Raoult’s Law: p A = x A p A * and p B = x B p B * = (1-x A )p B * iii. Henry’s Law: p B = x B K B b. Chemical potential and Ideal Solutions c. Entropy of Mixing, Free Energy of mixing i. Δ G mix = nRT(x A lnx A + x B lnx B Purely entropic, as in gas mixture. ii. Δ H mix = Δ G mix + T Δ S mix = 0 No enthalpy change, Δ G is due to entropy of mixing iii. mix mix T G V p ⎛⎞ ∂Δ Δ= = ⎜⎟ ⎝⎠ 0 No volume change, just like ideal gas d. Non ideal solutions i. Positive Deviations: Δ u > 0 (most common) Mixing is energetically not favorable in liquid phase
Background image of page 2
ii. Vapor pressure is higher than expected by Raoult’s Law iii. Can make same argument for negative deviation.
Background image of page 3

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

View Full DocumentRight Arrow Icon
Image of page 4
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 11/27/2011 for the course CHEM 5.43 taught by Professor Timothyf.jamison during the Spring '07 term at MIT.

Page1 / 5

final_exam_rev - MIT OpenCourseWare http:/ocw.mit.edu 5.60...

This preview shows document pages 1 - 4. Sign up to view the full document.

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