CAS CH 110 Lecture Notes - Lecture 31: Collision Theory, Boltzmann Distribution, Collision Frequency
25 Apr 2017
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Chain reactions have highly reactive intermediates that produce more highly reactive intermediates and so on. These reaction intermediate are called a chain carrier. The rate laws are very complex, and not derived here. The formation of hbr in the reaction takes place by a chain reaction. H2 (g) + br2 (g) 2 hbr(g) The first step called, intiation, produces chain carriers h and br , is heat hv is light. Br2 (g) ( or hv) br + br . The second step, propagation, creates more chain carriers, in this case radicals. The final step, termination, occures when two chain carriers combine to form products. The equilibrium constant for an elementary reaction is equal to the forward and reverse rate constants of the reaction, we can show k = k1 /k-1 k2 For a + b c + d rate = k1[a][b] C + d a + b rate = k-1[c][d] k1[a][b] = k-1[c][d]
