**Title: Calculating the Standard Enthalpy Change (ΔH⁰ᵣₓₙ) for a Reaction****Introduction:**In thermochemistry, one of the key concepts is the calculation of the enthalpy change (\(\Delta H\)) for a chemical reaction. This calculation helps understand the heat exchange involved in chemical processes. In this example, we will calculate the standard enthalpy change (\(\Delta H⁰ᵣₓₙ\)) for the reaction given below using the enthalpy changes of other related reactions.**Problem Statement:**Calculate \(\Delta H⁰ᵣₓₙ\) for the following reaction:\[ CS_2 (l) + 3O_2 (g) \rightarrow CO_2 (g) + 2SO_2 (g) \]**Given Reactions and Their Enthalpy Changes (\(\Delta H\)):**1. \[ C (s) + O_2 (g) \rightarrow CO_2 (g) \] - \(\Delta H = -393.5 \, \text{kJ}\)2. \[ S (s) + O_2 (g) \rightarrow SO_2 (g) \] - \(\Delta H = -296.8 \, \text{kJ}\)3. \[ C (s) + 2S (s) \rightarrow CS_2 (l) \] - \(\Delta H = +87.9 \, \text{kJ}\)**Explanation of the Provided Reactions:**1. The first given reaction describes the formation of carbon dioxide (\(CO_2\)) from solid carbon (\(C\)) and oxygen gas (\(O_2\)) with an enthalpy change (\(\Delta H\)) of -393.5 kJ.2. The second reaction details the formation of sulfur dioxide (\(SO_2\)) from solid sulfur (\(S\)) and oxygen gas (\(O_2\)) with an enthalpy change (\(\Delta H\)) of -296.8 kJ.3. The third reaction indicates the formation of carbon disulfide (\(CS_2\)), a liquid, from solid carbon (\(C\)) and solid sulfur (\(S\)) with an enthalpy change (\(\Delta H\

By rearranging the given equations and adjusting them to get the required equation will lead to…

Calculate AH°n for the first reaction shown from the remaining reactions. CS2(e) + 302(g) → CO2(g) + 25O2(g) AH°xn = ? %3D Given: C(s) +O2(g) – CO2(g) AH = -393.5 kJ S(s) + O2(g)-SO2(g) AH = -296.8 kJ Cls) + 2S(s)- CS2(@) AH = +87.9 kJ

Calculate AH°n for the first reaction shown from the remaining reactions. CS2(e) + 302(g) → CO2(g) + 25O2(g) AH°xn = ? %3D Given: C(s) +O2(g) – CO2(g) AH = -393.5 kJ S(s) + O2(g)-SO2(g) AH = -296.8 kJ Cls) + 2S(s)- CS2(@) AH = +87.9 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

**Title: Calculating the Standard Enthalpy Change (ΔH⁰ᵣₓₙ) for a Reaction**

**Introduction:**
In thermochemistry, one of the key concepts is the calculation of the enthalpy change (\(\Delta H\)) for a chemical reaction. This calculation helps understand the heat exchange involved in chemical processes. In this example, we will calculate the standard enthalpy change (\(\Delta H⁰ᵣₓₙ\)) for the reaction given below using the enthalpy changes of other related reactions.

**Problem Statement:**

Calculate \(\Delta H⁰ᵣₓₙ\) for the following reaction:
\[ CS_2 (l) + 3O_2 (g) \rightarrow CO_2 (g) + 2SO_2 (g) \]

**Given Reactions and Their Enthalpy Changes (\(\Delta H\)):**

1. \[ C (s) + O_2 (g) \rightarrow CO_2 (g) \]
- \(\Delta H = -393.5 \, \text{kJ}\)

2. \[ S (s) + O_2 (g) \rightarrow SO_2 (g) \]
- \(\Delta H = -296.8 \, \text{kJ}\)

3. \[ C (s) + 2S (s) \rightarrow CS_2 (l) \]
- \(\Delta H = +87.9 \, \text{kJ}\)

**Explanation of the Provided Reactions:**

1. The first given reaction describes the formation of carbon dioxide (\(CO_2\)) from solid carbon (\(C\)) and oxygen gas (\(O_2\)) with an enthalpy change (\(\Delta H\)) of -393.5 kJ.

2. The second reaction details the formation of sulfur dioxide (\(SO_2\)) from solid sulfur (\(S\)) and oxygen gas (\(O_2\)) with an enthalpy change (\(\Delta H\)) of -296.8 kJ.

3. The third reaction indicates the formation of carbon disulfide (\(CS_2\)), a liquid, from solid carbon (\(C\)) and solid sulfur (\(S\)) with an enthalpy change (\(\Delta H\

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