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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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### Thermochemistry Problem: Reaction Enthalpy Calculation The following reactions and their respective enthalpy changes (\( \Delta H \)) are given: 1. \(\frac{1}{2} \text{N}_2(g) + \text{O}_2(g) \rightarrow \text{NO}_2(g)\) \( \Delta H = 33.2 \, \text{kJ} \) 2. \(\text{NO}_2\text{Cl}(g) \rightarrow \text{NO}_2(g) + \frac{1}{2} \text{Cl}_2(g)\) \( \Delta H = 20.6 \, \text{kJ} \) ### Task Calculate the enthalpy change (\( \Delta H \)) for the following reaction: \[ \text{N}_2(g) + 2\text{O}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{NO}_2\text{Cl}(g) \] ### Solution To calculate the overall enthalpy change for this reaction, use Hess's law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step. 1. Reverse reaction 2: \[\text{NO}_2(g) + \frac{1}{2} \text{Cl}_2(g) \rightarrow \text{NO}_2\text{Cl}(g) \] Reverse \( \Delta H = -20.6 \, \text{kJ} \) 2. Adjust reaction 1 for two moles of \(\text{NO}_2(g)\): \[\text{N}_2(g) + 2\text{O}_2(g) \rightarrow 2\text{NO}_2(g)\] Adjusted \( \Delta H = 2 \times 33.2 = 66.4 \, \text{kJ} \) 3. Combine the adjusted reactions: \[\text{N}_2(g) + 2\text{O}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{NO}_2\text{Cl}(g)\] Calculate the total \( \Delta H \): \[ \Delta H = 66.4 \, \text
Transcribed Image Text:### Thermochemistry Problem: Reaction Enthalpy Calculation The following reactions and their respective enthalpy changes (\( \Delta H \)) are given: 1. \(\frac{1}{2} \text{N}_2(g) + \text{O}_2(g) \rightarrow \text{NO}_2(g)\) \( \Delta H = 33.2 \, \text{kJ} \) 2. \(\text{NO}_2\text{Cl}(g) \rightarrow \text{NO}_2(g) + \frac{1}{2} \text{Cl}_2(g)\) \( \Delta H = 20.6 \, \text{kJ} \) ### Task Calculate the enthalpy change (\( \Delta H \)) for the following reaction: \[ \text{N}_2(g) + 2\text{O}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{NO}_2\text{Cl}(g) \] ### Solution To calculate the overall enthalpy change for this reaction, use Hess's law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step. 1. Reverse reaction 2: \[\text{NO}_2(g) + \frac{1}{2} \text{Cl}_2(g) \rightarrow \text{NO}_2\text{Cl}(g) \] Reverse \( \Delta H = -20.6 \, \text{kJ} \) 2. Adjust reaction 1 for two moles of \(\text{NO}_2(g)\): \[\text{N}_2(g) + 2\text{O}_2(g) \rightarrow 2\text{NO}_2(g)\] Adjusted \( \Delta H = 2 \times 33.2 = 66.4 \, \text{kJ} \) 3. Combine the adjusted reactions: \[\text{N}_2(g) + 2\text{O}_2(g) + \text{Cl}_2(g) \rightarrow 2\text{NO}_2\text{Cl}(g)\] Calculate the total \( \Delta H \): \[ \Delta H = 66.4 \, \text
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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