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Problem 1. Assume that the reaction Оз + М > О2 + M is elementary and write down a plausible rate equation for dO3(t)/dt. O3 (t) is the concentration of ozone (mol/liter) at time t.

Problem 1. Assume that the reaction Оз + М > О2 + M is elementary and write down a plausible rate equation for dO3(t)/dt. O3 (t) is the concentration of ozone (mol/liter) at time t.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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I need help solving the following Physical chemistry kinetics problem using Wolfram Mathematica please. Please see the attached documents.

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Problem 1. Assume that the reaction Оз + М > 02 + M 2 is elementary and write down a plausible rate equation for dO3 (t)/dt. O3(t) is the concentration of ozone (mol/liter) at time t. Problem 2. Assume that you know that the reaction takes place in two steps 03 + M 2 02 +0+ M (1) and 0+ 03 → 2 02 (2) Here M is an inert molecule, such as nitrogen or argon. Write rate equations for all compounds in reaction; express dO3/dt, dO/dt and dO2/dt, in terms of the concentrations of O2, 03, 0, and M. Problem 3. Write the rate equations for the reactions 1 and 2 (given in problem 2) in terms of the extents of reactions.
Transcribed Image Text:Problem 1. Assume that the reaction Оз + М > 02 + M 2 is elementary and write down a plausible rate equation for dO3 (t)/dt. O3(t) is the concentration of ozone (mol/liter) at time t. Problem 2. Assume that you know that the reaction takes place in two steps 03 + M 2 02 +0+ M (1) and 0+ 03 → 2 02 (2) Here M is an inert molecule, such as nitrogen or argon. Write rate equations for all compounds in reaction; express dO3/dt, dO/dt and dO2/dt, in terms of the concentrations of O2, 03, 0, and M. Problem 3. Write the rate equations for the reactions 1 and 2 (given in problem 2) in terms of the extents of reactions.
Problem 4. Derive an equation for dO3(t)/dt by using the steady state approximation. Problem 5. The rate constants for these reactions have been measured and they are k = 2.2 1012 exp[- 2400(cal/mol)/RT] k-1 = 2.96 10' exp[890(cal/mol)/RT] k2 = 3.37 1010 exp[-5700(cal/mol)/RT] One activation energy is negative. Is that sensible? What does that suggest? If these numbers are correct is the steady state approximation correct if the temperature is 500 K ?
Transcribed Image Text:Problem 4. Derive an equation for dO3(t)/dt by using the steady state approximation. Problem 5. The rate constants for these reactions have been measured and they are k = 2.2 1012 exp[- 2400(cal/mol)/RT] k-1 = 2.96 10' exp[890(cal/mol)/RT] k2 = 3.37 1010 exp[-5700(cal/mol)/RT] One activation energy is negative. Is that sensible? What does that suggest? If these numbers are correct is the steady state approximation correct if the temperature is 500 K ?
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