When two speeding objects collide, the extent of damage that occurs depends on the speeds of the object and the position of impact. For the reaction of nitric oxide NO with chlorine Cl2, two approaches of collision A and Bare possible as shown in figure 6.13. It is clear that the first orientation in A favors the reaction while the orientation in B will not result in formation of the product NOCl.
Collision theory explains the temperature dependence of rate of a reaction based specifically on the concept of effective collisions. However, collision theory does not account for the role of activation energy influencing the rate of a reaction. Another theory that was proposed a few years later by Eyring, is the Transition State Theory.
Orientation Barrier
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As noted earlier, the rate of reaction also depends on p, the fraction of collisions that occur with proper orientation. This factor is independent of temperature. Why proper orientation of the reactant molecule is important can be understood from the figure.
fig 6.13 - Importance of molecular orientation in the reaction of NO and Cl
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