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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The ozone in the Earth’s ozone layer decomposes according to the equation

2 O3(g) → 3 O2(g)

The mechanism of the reaction is thought to proceed through an initial fast equilibrium and a slow step:

images

Show that the mechanism agrees with this experimental rate law:

Rate = −(1/2)Δ[O3]/Δt = k[O3]2[O2].

Interpretation Introduction

Interpretation:

From the given set of mechanisms it should be proved that the given rate law matches with the given steps.

Concept introduction:

Rate law or rate equation: Rate law:

It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

aA + bBxXRate of reaction = k [A]m[B]n

Order of a reaction:  The order of each reactant in a reaction is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.

Rate constant, k: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Explanation

Examining the given set of steps it is clear that step 2 is the slowest step which means that it is the rate determining step and the rate equation for that is as follows,

  Rate Law for Rate determing step,Rate = k[O3][O]FromStep1theKcvalueis as follows, Kc = [O2][O][O3][<

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