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
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**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\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a6e4794-5644-431d-9e96-b37fbaf0b60a%2F1c1c75af-ad82-4cff-aa17-b601063a0a08%2F4gvfxj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**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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