| |
| Recap |
| In
this Lecture you have learnt the following |
| |
Summary |
| |
In this lecture, you have been introduced to the transition state theory of reaction rates. This theory relates the rate constant to the activation parameters involved in the rate process, namely, the free energy, enthalpy and entropy of activation. |
| |
The concentration of the transition state is dependent on the reactant concentrations, and this proportionality constant K  is expressed in terms of the equilibrium constant K between the reactants and the transition state. This K is expressed in terms of the partition functions of reactants and the transition state and this equilibrium is rationalized through the population equilibration between the reactants and the transition state. Although the activated complex refers to the region on the potential energy diagram in the vicinity of the transition state (which is one point on the potential energy curve), the two terms are often used synonymously. The decomposition rate of the activated complex is related to a vibrational frequency of the transition state. Through this vibration, the activated complex is converted to the products. The steric factor P encountered in the collision theory is related to the steric or orientational entropy of activation, P = exp(  S steric/R). The effect of isotopic substation on the kinetics of deuteration is explained using the transition state theory. |
| |
|
| |
|
| |
Congratulations, you have finished Lecture . To view the next lecture select it from the left hand side menu of the page |
|
| |
| |
| |
| |
| |
| |
| |
| |
| |
| |
| |
| |
| |
| |
|
