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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

A The compound 1,3-butadiene (C4H6) forms 1,5-cyclooctadiene, C8H12 at higher temperatures.

C4H6(g) → ½ C8H12(g)

Use the following data to determine the order of the reaction and the rate constant, k. (Note that the total pressure is the pressure of the unreacted C4H6 at any time plus the pressure of the C8H12.)

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Interpretation Introduction

Interpretation:

For the given reaction the order and the rate constant should be determined using the given time and total pressure data.

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

Order of the reaction:

The given data table contains time and the respective total pressure.

The graph between total pressures with respect to time is plotted as below.

The reaction follows second order, since the graph plotted for reactant concentration with respect to time gives a straight line.

Calculation for the rate constant of the given reaction is determined as below,

Find the slope for any two values in the graph:

  slope=Δ[TotalPressure]&#

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