{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Lec-06-Chap13-2-Complete

Lec-06-Chap13-2-Complete - Lec-06-Chap13-2-Complete Lec-06...

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

View Full Document Right Arrow Icon
Lec-06-Chap13-2-Complete 9/15/2009 Chemical Kinetics Rect. Mechanisms. Arrhenius Eq., etc. 1 Rate Laws for Chemical Reactions Chemical reactions, described by stoichiometric “overall” equations: + A C D B c d a b The overall reaction equation describes the identity and proportions in which the reactant species are consumed and the identity and proportions in which the product species are generated . 1 Lec-06: Reaction Mechanism and Rate Laws Chapter 13 Rate Laws - continued     rate constant A 1 rat A B = e m t t n t d t k a dt The rate law , frequently of the form reflects instead the detailed series of elementary reaction steps by which the chemical reaction proceeds . Consider the reaction   2 2 3 2 2 2 I aq H O aq 2H O I aq 4H O The rate law is found experimentally to be   2 2 I rate H O t t k t 2 If it was based on the overall balanced equation we would guess 2 2 2 2 3 rate(t) I H O H O k
Image of page 1

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

View Full Document Right Arrow Icon