   Chapter 14, Problem 37PS

Chapter
Section
Textbook Problem

Calculate the activation energy, Ea, for the reaction2 N2O5(g) → 4 NO2(g) + O2(g)from the observed rate constants: k at 25 °C = 3.46 × 10−5 s−1 and k at 55 °C = 1.5 × 10−3 s−1.

Interpretation Introduction

Interpretation:

For the given reaction under given reaction conditions the activation energy for the reaction should be determined.

Concept Introduction:

Arrhenius equation:

Arrhenius equation is used to calculate the rate constant of many reactions. Arrhenius equation takes the form

k=Ae-Ea/RT

Where,

k=rate constant

A=frequency factor

e=base of logarithms

Ea = energy of activation

T=Temperature

Mathematically, the above equation can be written as,

lnk=lnA-EaRT

Explanation

Given,

ln(K1K2)=EaR(1T2-1T1)T1=25C=298.15KT2=55C=328.15KK1=3.46×10-5s1K2= 1.5×10-3s1Ea=?

In order to determine the activation energy for the given reaction we need to use the following expression which relates the rate constant, activation energy and the temperature.

ln(K1K2)=EaR(1T2-1T1)Ea=

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