MadSci Network: Chemistry |
First we need to nail down exactly what we mean by "order". The order of the reaction is not determined by concentration; rather, it is how much of an effect the concentration of a species has on the reaction that determines the order. Here is the reaction you are studying: 2 H2O2 -----(I-)-----> 2 H2O + O2 Iodine does not show up in the overall equation, as it is a catalyst. Its concentration, however, is still important to the overall rate. The rate equation can't be determined just by looking at the equation. It must be determined experimentally. Ira Levine in "Physical Chemistry" (2nd edition) obligingly provides it for us: r = k[H2O2][I-] The 'overall order' of the reaction is determined by adding up the superscripts on each component; here, each one is equal to 1. If the reaction depended only on the peroxide concentration, the rate equation would be r = k[H2O2] and the reaction would be first order. The reaction depends on *both* concentrations, though, and neither concentration term is raised to any power other than 1. Thus, this is a second-order reaction.
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