This preview shows page 1. Sign up to view the full content.
Unformatted text preview: = ∗ = !"#$%&$'#
(5 points each)
b) The rate constant for a bimolecular reaction, which has units of cm3 s-1 (so you would multiply by two densities to get a rate), is predicted
by simple collision dynamics to be !!! !"
ℳ = 2 ! ! Use this equation to define the frequency factor A in the Arrhenius equation in terms of measureable variables. Here, d is the
molecular diameter and ℳ is the molar mass. = 2 ! !
c) ℳ (10 points) Use the substitutions E = ½ mv2 and kB = R/NA to rewrite the Boltzmann distribution, provided below in a suggestive form that shows its
connection to the Arrhenius equation. Remember to substitute for dv as well, where dE = mv dv. Also substitute Emol for E*NA to
account for the fact that the units of Ea in the Arrhenius equation are J/mol*K as it is referring to the energy of a mole of particles. = 2! !!! ! /!!! ! !" !"
! = !"
! = ! ! = ! d) !"# = !!!! !
!! !!"#$! !
! !!"#!!"# !!! ! /!!...
View Full Document
This test prep was uploaded on 04/03/2014 for the course CHEM 1b taught by Professor Heath,rees during the Spring '13 term at Caltech.
- Spring '13
- Organic chemistry