### Calculation of the Standard Enthalpy of Reaction (\(\Delta H_{\text{rxn}}\)) for the Preparation of Nitrous Acid, HNO\(_2\)To calculate the standard enthalpy of reaction (\(\Delta H_{\text{rxn}}\), in kJ/mol) for producing nitrous acid, using the given thermodynamic data:**Reaction for Preparation of Nitrous Acid:**\[ \text{HCl(g)} + \text{NaNO}_2(\text{s}) \rightarrow \text{HNO}_2(\text{l}) + \text{NaCl(s)} \]**Thermodynamic Reactions and Enthalpy Changes (\(\Delta H\)):**1. **\[ 2\text{NaCl(s)} + \text{H}_2\text{O(l)} \rightarrow 2\text{HCl(g)} + \text{Na}_2\text{O(s)} \]** - \(\Delta H = 507.31 \, \text{kJ/mol}\)2. **\[ \text{NO(g)} + \text{NO}_2\text{(g)} + \text{Na}_2\text{O(s)} \rightarrow 2\text{NaNO}_2(\text{s)} \]** - \(\Delta H = -427.14 \, \text{kJ/mol}\)3. **\[ \text{NO(g)} + \text{NO}_2\text{(g)} \rightarrow \text{N}_2\text{O(g)} + \text{O}_2(\text{g)} \]** - \(\Delta H = -42.68 \, \text{kJ/mol}\)4. **\[ 2\text{HNO}_2\text{(l)} \rightarrow \text{N}_2\text{O(g)} + \text{O}_2(\text{g)} + \text{H}_2\text{O(g)} \]** - \(\Delta H = 34.35 \, \text{kJ/mol}\)5. **\[ \text{H}_2\text{O(l)} \rightarrow \text{H}_2\text{O(g)} \]** - \(\Delta H = 44.012 \, \text{kJ/mol}\)Each

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2. Please calculate the standard enthalpy of reaction (AHxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s)→ HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na₂O(s) → 2NaNO₂(s) NO(g) + NO2(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O₂(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ 507.31 kJ/mol AH-427.14 kJ/mol AH = -42.68 kJ/mol ΔΗ = 34.35 kJ/mol ΔΗ 44.012 kJ/mol

2. Please calculate the standard enthalpy of reaction (AHxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s)→ HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na₂O(s) → 2NaNO₂(s) NO(g) + NO2(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O₂(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ 507.31 kJ/mol AH-427.14 kJ/mol AH = -42.68 kJ/mol ΔΗ = 34.35 kJ/mol ΔΗ 44.012 kJ/mol

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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