Hydrogen peroxide disproportionates to water and molecular oxygen in the presence of iodide in neutr — Kinetics Chemistry Question
Question
Hydrogen peroxide disproportionates to water and molecular oxygen in the presence of iodide in neutral solution according to a mechanism consisting of two elementary steps:
H2O2(aq) + I–(aq) IO–(aq) + H2O(l) reaction 1
H2O2(aq) + IO–(aq) I–(aq) + O2(g) + H2O(l) reaction 2
The rate constant for reaction 1 is much larger than the rate constant for reaction 2. Which statement is correct?
A.✓ Correct
As the reaction proceeds, the predominant form of iodine in solution is IO–(aq).
B.
Adding more iodide to the reaction will not increase the rate of production of O2.
C.
The reaction is zeroth-order in H2O2.
D.
The reaction will go more slowly at higher O2 pressures.
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