Lecture36A - Lecture 36 1 Reaction Dynamics: Cross-Sections...

Info iconThis preview shows pages 1–3. 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
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Lecture 36 1 Reaction Dynamics: Cross-Sections (Chapter 30.1-4) We are now ready to combine our knowledge of gas-phase kinetics with kinetic gas theory. As I said earlier, two molecules cant react unless they collide. Therefore the bimolecular rate constant, must be related to the binary collision rate, Z AB . For an elementary bimolecular reaction: [ ] [ ][ ] Products, v k d A A B k A B dt + = - = First lets assume that the reaction can occur if we have a hard-sphere collision. We have already learned that -1 3-1 AB 3-1-1 3 3 1/2 2 AB Since k has units of sec dm mol and has units of m molec sec , this is easy to fix: 1000 8 where and and 2 r A AB r A B B A B r A u dm molec k N u m mol d d k T m m u m m = + = = = + B v AB AB r A B Z u = = Lecture 36 2 How well does this work for a very reactive binary collision? ( 29 ( 29 5 3-1-1 3 2 2 7.59 10 dm mol sec k O g O g O k + = 3 3 o o O 3 O 2 2 o 19 2 1/2 For O, 1.80A; For O , 5.16A 38A 3.8 10 2 8 at 298K 725 / O O B r d d d d m k T u m s - = = + = = = = = 11 3-1 -1 1.66 10 dm mol s1....
View Full Document

Page1 / 8

Lecture36A - Lecture 36 1 Reaction Dynamics: Cross-Sections...

This preview shows document pages 1 - 3. Sign up to view the full document.

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