Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ...
Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ... Physical Chemistry 3: — Chemical Kinetics — - Christian-Albrechts ...
7.1 Foundations of transition state theory 153 ∆ ‡ : Born-Oppenheimer potential energy barrier (7.30) ∆ 0 : zero-point corrected threshold energy for the reaction (7.31) : Arrhenius activation energy (7.32) ∆ 0 is given with respect to the zero-point energies of the reactants and the TS, = 1 2 X (7.33) 7.1.4 Tolman’s interpretation of the Arrhenius activation energy I We now understand the difference between E and ∆E 0 : 2 ln ( ) = Ã = 2 ln ‡ µ exp = ∆ 0 + + 2 ln ‡ − | {z } =h reacting moleculesi − ∆ 0 (7.34) ! (7.35) µ 2 ln + 2 ln (7.36) | {z } =h all molecules i • ∆ 0 is difference of the zero-point levels of the reactants and the TS, • the term is the mean translational energy in the RC (from the factor), • the 2 ln terms are the internal (vibration-rotation) energies of the TS and the reactants, respectively. y I Tolman’s interpretation of E (see Fig. 7.4): = h reacting molecules i − h all molecules i (7.37)
7.2 Applications of transition state theory 154 7.2 Applications of transition state theory ( )= ‡ µ exp − ∆ 0 (7.38) TST has gained enormous importance in all areas of physical chemistry because it provides the basis for understanding – and/or calculating – • quantitative values of preexponential factors, • ∆ 0 from measured values, • -dependence of and deviations from Arrhenius behavior, • gas phase and liquid phase reactions (proton transfer, electron transfer, organic reactions, reactions of ions in solutions), • pressure dependence of reaction rate constants (activation volumes), • kinetic isotope effects, • structure-reactivity relations (e.g., Hammett relations in organic chemistry), • features of biological reactions (enzyme reactions), • heterogeneous reactions (heterogeneous catalysis, electrode kinetics), . . . 7.2.1 The molecular partition functions In order to evaluate Eq. 7.29 for a given reaction, we need, besides ∆ 0 , the molecular partition functions for the reactants and the TS. We summarize only the main points here; further information is given in Appendix G. I Definition: = P − (7.39) I Physical interpretation: • The molecular partition function is a number which describes how many states are available to the molecule at a given temperature . • The ratio ‡ (7.40) in Eq. 7.29 is thus the ratio of the number of states available to the TS and ‡ the reactant molecules. Since each state is equally likely, is the relative probability of the TS vs. the probability of the reactants. Note again that ‡ motion along the RC. is the partition function of the TS excluding the translational
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7.1 Foundations of transition state theory 153<br />
∆ ‡ : Born-Oppenheimer potential energy barrier (7.30)<br />
∆ 0 : zero-point corrected threshold energy for the reaction (7.31)<br />
: Arrhenius activation energy (7.32)<br />
∆ 0 is given with respect to the zero-point energies of the reactants and the TS,<br />
= 1 2<br />
X<br />
(7.33)<br />
7.1.4 Tolman’s interpretation of the Arrhenius activation energy<br />
I We now understand the difference between E and ∆E 0 :<br />
2 ln ( )<br />
= <br />
<br />
Ã<br />
= 2 <br />
ln <br />
<br />
<br />
‡ µ<br />
<br />
exp<br />
<br />
= ∆ 0 + + 2 ln ‡ <br />
−<br />
| {z }<br />
=h reacting moleculesi<br />
− ∆ 0<br />
<br />
(7.34)<br />
! (7.35)<br />
µ<br />
2 ln <br />
+ 2 ln <br />
<br />
(7.36)<br />
<br />
<br />
| {z }<br />
=h all molecules i<br />
• ∆ 0 is difference of the zero-point levels of the reactants and the TS,<br />
• the term is the mean translational energy in the RC (from the factor),<br />
• the 2 ln terms are the internal (vibration-rotation) energies of the TS and<br />
<br />
the reactants, respectively. y<br />
I Tolman’s interpretation of E (see Fig. 7.4):<br />
= h reacting molecules i − h all molecules i (7.37)