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For a reaction2H2O2\(\frac{I^-}{\text{alkaline medium}}\to\)2H2O+O2 the proposed mechanism is as given below: (I) H2O2 + I– → H2O + IO– (slow) (II) H2O2 + IO– → H2O + I– + O2 (fast) (a) Write rate law for the reaction. (b) Write the overall order of reaction. (c) Out of steps (I) and (II), which one is rate determining step? |
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Answer» The reactions given are as follows: 2H2O2\(\frac{I^-}{\text{alkialine medium}}\to\)2H2O+O2 H2O2+I-→H2O+IO-(slow) (i) H2O2+IO-→H2O+I-+O2 (fast) (ii) (a) To find the rate expression, we consider rate determining step, which is step (I) for this reaction. Then according to the rate law, Rate=k[H2O2][I-] (b) Since, two reagents are involved in the rate-limiting step, thus overall rate of reaction is proportional to the concentration of those reagents, that is, 2. (c) The slowest step in this reaction is called the rate-determining step, that is step (I). |
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