01:160:162 Lecture 5: lecture 5sf
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H2o2 decomposes by first order kinetics with a half life of 20. 0 minutes. Or: 3. 47 x 10-3 (0. 100) = 3. 47 x 10-3 m min-1. Assume that the above reaction is 2nd order. To solve for the rate at any concentration: = kc2 = (0. 100)(0. 150)2 = 2. 25 x 10-3 m min-1. Effect of temperature on rate aa + bb products. This equation shows how rate depends on concentration. In general, a higher temperature means a faster reaction. Although temperature is not explicitly in the rate equation, the rate constant k is temperature dependent. So, as temperature increases, k increases, and thus the rate will also increase. react, they must have an encounter a collision. A collision is a necessary but not a sufficient condition for a reaction of two different species. If there is a reaction, there must have been a collision.