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OpenStudy (anonymous):
An oxidation is described by the following balanced equation. Calculate the rate of formation for I3- when the [H2O2] = 0.300 M and [I-] = 0.400 M
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OpenStudy (anonymous):
H2O2 + 3I- + 2H+ -> I3- + 2H2O
OpenStudy (anonymous):
I've calculated the reaction rate and the rate constant. I'm just wondering how to take in account the 2H2O when finding the rate of reaction for I3-
OpenStudy (anonymous):
rate of formation that is.
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