{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

lecnotes19 - MIT OpenCourseWare http/ocw.mit.edu 5.111...

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 5.111 Principles of Chemical Science Fall 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 Document Right Arrow Icon
reactants 19.1 5.111 Lecture Summary #19 CHEMICAL EQUILIBRIUM (Chapter 9 Section 9.0-9.9) Topics Nature of Chemical Equilibrium Meaning of K Relationship between Equilibrium Expressions External Effects on K Chemical reactions reach a state of dynamic equilibrium in which the rates of forward and reverse reactions are equal and there is no net change in composition. Consider: N 2 (g) + 3H 2 (g) 2NH 3 (g) G° = -32.90 kJ/mol conc time When the reaction mixture has not produced enough products to have reached equilibrium, the spontaneous direction of change is toward more products ( G forward reaction ___ 0). When excess products are present (ex. pure ammonia), the reverse reaction is spontaneous ( G forward reaction ______ 0). Progress of reaction Free energy, G Pure Pure products G < 0 G = 0 G > 0
Background image of page 2
19.2 The reaction free energy ( G) changes as the proportion of reactants and products change. To find out how G changes with composition of reactants and products, we need to know how the
Background image of page 3

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

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

{[ snackBarMessage ]}