Respuesta :
The intermediate of the reaction is [tex]OI^{-}[/tex]. The intermediate involves slow step and intermediates are stable.
What is intermediate of a reaction ?
Reaction intermediate is a substance which appears in the middle step of a chemical reaction. An intermediate always formed in an first elementary step and consumed in a next elementary step.
A mechanism for the reaction with a slow step followed by a fast step:
Step 1: [tex]H_{2}O_{2} (aq) + I^{-} (aq)[/tex] → [tex]H_{2}O(l) + OI^{-} (aq)[/tex] (Slow)
Step 2: [tex]H_{2}O_{2} (aq) + OI^{-} (aq)[/tex] → [tex]H_{2}O (l) + O_{2} (g) + I^{-} (aq)[/tex] (Fast)
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Overall Equation: [tex]2H_{2}O_{2}[/tex] → [tex]2H_{2}O + O_{2}[/tex]
Here the slow step is called the rate determining step. We can see that Step 1 is the slowest step in the given reaction so Step 1 is the rate determining step. The formation of intermediate is the slowest step. Reactants are not intermediates. The overall order of the reaction is 2.
[tex]OI^{-}[/tex] is the intermediate and [tex]I^{-}[/tex] is the catalyst.
Rate = rate of slow step = [tex]k [H_{2}O_{2}] [I^{-}][/tex].
Thus we can conclude that in the given reaction [tex]OI^{-}[/tex] is the intermediate.
Learn more about the Chemical reaction here: https://brainly.com/question/11231920
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