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: step1 slow: H202IH20oI (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 k[A]m[B]n , where '1, is understood (so don't write it) for m, n etc.) Rate

Explanation / Answer

Q1.

add both step reactions

H2O2 + I- + H2O2 + OI- = H2O + OI- + H2O + O2 + I-

get rid of common ions

2H2O2 + =2H2O + O2

Q2

catalyst --> are present initially and will be re-generated, this is I-

Q3

intermediates form and react, in this case, OI- is formed and then is reacted

Q4

Rate = k*[reactants]^r

note that we use the SLOWESt step since this determines reaction

Rate = k*[H2O2][I-]

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