The decomposition of hydrogen peroxide in the presence of potassium iodide is be

Question

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism tep1 slow: H,02+rHo+or step 2 .fast: H202 + or.- H2O + O2-r (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank (2) Which species acts as a catalyst? Enter formula. If none, leave box blank (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank 4) Complete the rate law for the overall reaction that is consistent with this mechanism (Use the form klA] IBI"... , where ' ) for m, n etc.) 'is understood (se don't write it Rate

Explanation / Answer

1)

overall reaction can be obtained by adding both the steps

H2O2 + I- + H2O2 + OI- —> H2O + OI- + H2O + O2 + I-

After removing common species from reactant and product side

2 H2O2 —> 2 H2O + O2

2)

I- is catalyst because it is used in 1st step and produced back in last step

3)

OI- is an intermediate because it is produced in 1st step and used up in next step

4)

rate depends on the slowest step

here 1st step is slowest step

So, rate law is:

rate = k [H2O2][I-]

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