Problem: Consider the following reaction: 2O3(g) → 3O2(g). The rate law for this reaction is as follows: Rate = k[O3]2/[O2]Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?

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We are asked to determine what fraction of the O3 will have reacted when the rate falls to one-half of its initial value.


Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


Given:            

Rate=k[O3]2[O2]

[O3] = 1.0 mol

[O2] = 1.0 mol

Volume of Container = 1 L

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Problem Details
Consider the following reaction: 2O3(g) → 3O2(g). The rate law for this reaction is as follows: Rate = k[O3]2/[O2]

Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?
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