The rate of decomposition of hydrogen peroxide can be increased by having the re

Question

The rate of decomposition of hydrogen peroxide can be increased by having the reaction occur in the presence of iodide ion. The reaction is thought to proceed by a two step mechanism:

Step 1: H2O2 + I- --> H2O + IO-

Step 2: IO- + H2O2 --> H2O + O2 + I-

a. Write the rate law for each step of the mechanism.

b. Write the chemical reaction for the overall equation.

c. Identify the chemical species that acts as a catalyst. Is it heterogeneous or homogeneous? Identify the chemical species that is an intermediate.

d. What about the mechanism allows you to distinguish between a catalyst and an intermediate?

e. If the reaction is first order in both hydrogen peroxide and iodide ion, which step of the mechanism should be labeled as rate determining?

Explanation / Answer

for step 1,rate law is given by r1 =k1 [ H2O2 ][I- ]
for step 2,rate law is given by,r2 =k2[IO- ][H2O2 ]
overall reaction is given by
2H2O2 -->2 H2O +O2
IO- and I- are intermediate


                   

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