Derive an integrated rate law for the parallel reaction (competing reaction) ? → ? ??? ? → ?.Both reactions are first order with respect to A. Derive equations both for [A] as a function of t and [C] as a function of t.The rate constant, k, is 42.6 dm3 mol-1 s-1 for the following gas-phase reaction at 32oC. 2NO2 + Cl2 → 2NO2ClThe reaction is first order in NO2 and first-order in Cl2. Calculate the number of moles of NO2, Cl2, and NO2Cl present after 10.0 s if 2.00 mol of NO2 is mixed with 3.00 mol of Cl2 in a 400-dm3 vessel at 32°C. k1Derive an integrated rate law for the parallel reaction (competing reaction) A → C and A – D.Both reactions are first order with respect to A. Derive equations both for [A] as a function of tand [C] as a function of t.The rate constant, k, is 42.6 dm³ mol-1 s-1 for the following gas-phase reaction at 32°C.2NO2 + Cl2 → 2NO2C1The reaction is first order in NO2 and first-order in Cl2. Calculate the number of moles of NO2,Cl2, and NO2CI present after 10.0 s if 2.00 mol of NO2 is mixed with 3.00 mol of Cl2 in a 400-dm3vessel at 32°C.

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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

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Derive an integrated rate law for the parallel reaction (competing reaction) ? → ? ??? ? → ?.

Both reactions are first order with respect to A. Derive equations both for [A] as a function of t and [C] as a function of t.
The rate constant, k, is 42.6 dm3 mol-1 s-1 for the following gas-phase reaction at 32oC. 2NO2 + Cl2 → 2NO2Cl

The reaction is first order in NO2 and first-order in Cl2. Calculate the number of moles of NO2, Cl2, and NO2Cl present after 10.0 s if 2.00 mol of NO2 is mixed with 3.00 mol of Cl2 in a 400-dm3 vessel at 32°C.

k1
Derive an integrated rate law for the parallel reaction (competing reaction) A → C and A – D.
Both reactions are first order with respect to A. Derive equations both for [A] as a function of t
and [C] as a function of t.
The rate constant, k, is 42.6 dm³ mol-1 s-1 for the following gas-phase reaction at 32°C.
2NO2 + Cl2 → 2NO2C1
The reaction is first order in NO2 and first-order in Cl2. Calculate the number of moles of NO2,
Cl2, and NO2CI present after 10.0 s if 2.00 mol of NO2 is mixed with 3.00 mol of Cl2 in a 400-dm3
vessel at 32°C.

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