CHEM 1110 Lecture Notes - Lecture 8: Montreal Protocol, Rate Equation, Activated Complex
17 Mar 2017
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Kinetic theory of gases: 25 c, 1 atm, freque: 4. 1* 10^9. If every collision lead to reaction, would complete with 10^-9 s. Therefore: not every collision leads to reaction. A: pre exponential a factor: frequency factor. E^(-ea/rt): fraction of collisions where activation barrier can be surmounted. Partial breakage of no bond requires energy. Noco: tiniest motion of o toward co irreversibly lead to products. Even if there is sufficient energy, not necessarily a reaction. Must be aligned in very specific way for reaction to occur. Can determine ea if k is known at two temperatures lnk=ln a -(ea/r) (1/t) Sequence of elementary steps that show reaction path. One step is slower than the others and determines that overall reaction rate. Rate law of rds determines overall rate law. First step is slower than second: ea is larger. First step rate law=rate law of overall. Substances that increase the rate of reaction without being consumed.
