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1/2 N2(g) + O:(g) → NO:(g) AH = 33.2 kJ NO:CI(g) → NØ(g) + /2C12(g) AH = 20.6 kJ %3D Calculate the AH for the reaction: N2(g) + 202(g) + Cl2(g) → 2NO2CI(g) AH =?

1/2 N2(g) + O:(g) → NO:(g) AH = 33.2 kJ NO:CI(g) → NØ(g) + /2C12(g) AH = 20.6 kJ %3D Calculate the AH for the reaction: N2(g) + 202(g) + Cl2(g) → 2NO2CI(g) AH =?

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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1/2 N2(g) + O:(g) → NO:(8) AH = 33.2 kJ NO2CI(g) → NØ2(g) + 1/2C12(g) AH = 20.6 kJ Calculate the AH for the reaction: N2(g) + 202(g) + Cl2(g) → 2NO2CI(g) AH =?
Transcribed Image Text:1/2 N2(g) + O:(g) → NO:(8) AH = 33.2 kJ NO2CI(g) → NØ2(g) + 1/2C12(g) AH = 20.6 kJ Calculate the AH for the reaction: N2(g) + 202(g) + Cl2(g) → 2NO2CI(g) AH =?
Expert Solution
Step 1

The change in enthalpy for the reaction mentioned is to be calculated.

Step 2

Consider the following notations:-

F = Change in enthalpy of the 1st reaction

Q = Change in enthalpy of the 2nd reaction

Z = Change in enthalpy of the overall reaction

 

 

Step 3

The 1st reaction is given as:-

                                12N2 (g) + O2(g) → NO2 (g)                                             ....... (1)

Multiplying the reaction (1) with 2,

                                  N2 (g) + 2O2(g) → 2NO2 (g)                                           ....... (2)

The given enthalpy of the 1st reaction will also get multiplied by 2. Thus,

                                  F = 2 × 33.2 kJF = 66.4 kJ

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