When peroxide A is heated to 60 degree C in an inert solvent, it decomposes by a

Question

When peroxide A is heated to 60 degree C in an inert solvent, it decomposes by a first-order process. An initial concentration of 5.0 mmol/liter of peroxide changes to 4.0 mmol/liter after 1.0 h. In the following system, what fraction of the monomer should remain unconverted after 10 min at 60 degree C? What is the concentration of initiator after 10 min? System parameters (all at 60 degree C): k_p = 1.8 times 10^4 liter/mol s k_i, = 1.45 times 10^7 liter/mol s Initiator concentration = 4.0 times 10^-4 mol/liter

Explanation / Answer

The data you have provided for the question is not very clear. In part (a) you have not given any initial conc. for the monomer, and the question says "In the following system", but it is not clear which system is being talked about.

Nevertheless I am providing a solution based on first order reaction mechanism

For a first order reaction, the main equation is:

C = Co*e-kt

Here, Co is initial conc. and C is conc. at any time t, and k is rate constant

Putting values given for the peroxide, we get:
k = 6.19*10-5 s-1 for the peroxide

In part (b) what are the parameters kp and ki. Kindly clarify so that I can give you a prope solution.

Revert back asap.

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