2. The rate law expression determined above can be used to evaluate proposed mechanisms for this hydrogen peroxide decomposition reaction. Any valid mechanism must be consistent with the rate expression. For example, a catalyst such as the I used here does not appear in the overall chemical equation, but if its concentration shows up in the rate expression, it must be a part of the mechanism at some step. A two-step mechanism suggested for the present reaction is: H₂O2 + H₂O + IO (slow) IO + H₂O2 →→ O2+ H₂O + I (fast) Is this a valid mechanism? Is it consistent with the rate expression? Consistent with the stoichiometry of the reaction? What role does 10 play in the mechanism?

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2. The rate law expression determined above can be used to evaluate proposed mechanisms for this hydrogen peroxide decomposition reaction.
Any valid mechanism must be consistent with the rate expression. For example, a catalyst such as the I used here does not appear in the
overall chemical equation, but if its concentration shows up in the rate expression, it must be a part of the mechanism at some step.
A two-step mechanism suggested for the present reaction is:
H₂O2 + I¯¯ →→→→H₂O + IO (slow)
IO + H₂O2 →→ O2 + H₂O + I¯¯ (fast)
Is this a valid mechanism? Is it consistent with the rate expression? Consistent with the stoichiometry of the reaction? What role does 10 play
in the mechanism?
Normal
B|I\U
X₂ X² →
The valid mechanism would be rate = k [H₂0₂][1].
131313
fx l
3. If we are actually studying this roaction by the method of initial
BE
Saved
Tx
OG
Transcribed Image Text:2. The rate law expression determined above can be used to evaluate proposed mechanisms for this hydrogen peroxide decomposition reaction. Any valid mechanism must be consistent with the rate expression. For example, a catalyst such as the I used here does not appear in the overall chemical equation, but if its concentration shows up in the rate expression, it must be a part of the mechanism at some step. A two-step mechanism suggested for the present reaction is: H₂O2 + I¯¯ →→→→H₂O + IO (slow) IO + H₂O2 →→ O2 + H₂O + I¯¯ (fast) Is this a valid mechanism? Is it consistent with the rate expression? Consistent with the stoichiometry of the reaction? What role does 10 play in the mechanism? Normal B|I\U X₂ X² → The valid mechanism would be rate = k [H₂0₂][1]. 131313 fx l 3. If we are actually studying this roaction by the method of initial BE Saved Tx OG
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