The rate law for a certain process is given by
d[I2]/dt=k[Fe(CN)63-]2[I-]2[Fe(CN)64-]-1[I2]0
The overall reaction is given by
2Fe(CN)63- + 2I- = 2Fe(CN)64- + I2
Using this information, suggest a mechanism for this process and show how it leads to the overall reaction and the rate law given. (the order of reaction with respect to one substance indicates a pre-equilibrium in process). Don't forget the intermediate.
2Fe(CN)63- + 2I- 2Fe(CN)64- + I2
(Fe(CN)63- + e- Fe(CN)64-) x 2
2I- I2 + 2e-
2Fe(CN)63- + 2e- 2Fe(CN)64-
2Fe(CN)63- + 2I- 2Fe(CN)64- + I2
Rate laws must be determined experimentally; they cannot be predicted from the coefficients of balanced chemical equations. Every reaction is made up of a series of one or more elementary steps, and the rate laws and relative speeds of these steps will dictate the overall rate law. Indeed, the rate law for a reaction can be determined from its mechanism.
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