**Calculating ΔHrxn Using Given Reactions****Objective**: Calculate the enthalpy change (ΔHrxn) for the reaction:\[ 2\text{NOCl}(g) \rightarrow \text{N}_2(g) + \text{O}_2(g) + \text{Cl}_2(g) \]**Using the following set of reactions**:1. \( \frac{1}{2} \text{N}_2(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{NO}(g) \) \( \Delta H_{\text{rxn}} = 90.3 \, \text{kJ} \)2. \( \text{NO}(g) + \frac{1}{2} \text{Cl}_2(g) \rightarrow \text{NOCl}(g) \) \( \Delta H_{\text{rxn}} = -38.6 \, \text{kJ} \)**Instructions**: Enter your calculated value in the provided box in kJ.[Box for answer]: _____ kJBe sure to apply Hess's Law and manipulate the given reactions to derive the overall enthalpy change for the target reaction. Remember to adjust the coefficients and reverse reactions as necessary, adjusting their ΔHrxn values accordingly.

Using Hess's law, From the intermediate reactions we can the final reaction. 1/2N2 + 1/2 O2 --->…

Answered: 2NOC(g)N2g) + O2(g) + Cl2(g) given the…

2NOC(g)N2g) + O2(g) + Cl2(g) given the following set of reactions: 1/2 N2(g) + 1/2 O2(g)NO(g) NO(g) + 1/2 Cl,(g) NOCI(g) AH, 90.3 kJ %3D AH =-38.6 kJ kJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Calculating ΔH<sub>rxn</sub> Using Given Reactions**

**Objective**: Calculate the enthalpy change (ΔH<sub>rxn</sub>) for the reaction:

\[
2\text{NOCl}(g) \rightarrow \text{N}_2(g) + \text{O}_2(g) + \text{Cl}_2(g)
\]

**Using the following set of reactions**:

1. \( \frac{1}{2} \text{N}_2(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{NO}(g) \)
\( \Delta H_{\text{rxn}} = 90.3 \, \text{kJ} \)

2. \( \text{NO}(g) + \frac{1}{2} \text{Cl}_2(g) \rightarrow \text{NOCl}(g) \)
\( \Delta H_{\text{rxn}} = -38.6 \, \text{kJ} \)

**Instructions**: Enter your calculated value in the provided box in kJ.

[Box for answer]: _____ kJ

Be sure to apply Hess's Law and manipulate the given reactions to derive the overall enthalpy change for the target reaction. Remember to adjust the coefficients and reverse reactions as necessary, adjusting their ΔH<sub>rxn</sub> values accordingly.

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