Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Topic: Calculating the Enthalpy Change for Combustion
**Objective:**
To calculate the enthalpy change (in kJ/mol) for the combustion of carbon disulfide (CS₂) using the enthalpy values provided.
---
**Combustion Reaction:**
\[ \text{CS}_2 (\ell) + 3\text{O}_2 (g) \rightarrow \text{CO}_2 (g) + 2\text{SO}_2 (g) \]
---
**Enthalpy Values:**
| Reaction | \( \Delta H \) in kJ/mol |
|----------------------------------------------|---------------------------|
| \( \text{C} (s) + \text{O}_2 (g) \rightarrow \text{CO}_2 (g) \) | \(-393.6\) |
| \( \text{S} (s) + \text{O}_2 (g) \rightarrow \text{SO}_2 (g) \) | \(-296.8\) |
| \( \text{C} (s) + 2\text{S} (s) \rightarrow \text{CS}_2 (\ell) \) | \(+87.9\) |
---
**Explanation:**
- The table lists three reactions and their associated enthalpy changes, \( \Delta H \).
- The first reaction involves carbon reacting with oxygen to form carbon dioxide, releasing \(393.6 \, \text{kJ/mol}\).
- The second reaction involves sulfur reacting with oxygen to form sulfur dioxide, releasing \(296.8 \, \text{kJ/mol}\).
- The third reaction shows the formation of carbon disulfide from its elements, with an associated enthalpy change of \(+87.9 \, \text{kJ/mol}\).
**Instructions:**
To find the enthalpy change for the combustion of CS₂, apply Hess's Law, which involves manipulating the given reactions to derive the target reaction, ensuring the \( \Delta H \) values align correctly.](https://content.bartleby.com/qna-images/question/7c267e61-5731-4973-bfb7-6ab165a055a1/a1e27a15-367c-44bb-9b9d-61ff3a0fc9b2/0zqgc4m_processed.jpeg)
Transcribed Image Text:### Topic: Calculating the Enthalpy Change for Combustion
**Objective:**
To calculate the enthalpy change (in kJ/mol) for the combustion of carbon disulfide (CS₂) using the enthalpy values provided.
---
**Combustion Reaction:**
\[ \text{CS}_2 (\ell) + 3\text{O}_2 (g) \rightarrow \text{CO}_2 (g) + 2\text{SO}_2 (g) \]
---
**Enthalpy Values:**
| Reaction | \( \Delta H \) in kJ/mol |
|----------------------------------------------|---------------------------|
| \( \text{C} (s) + \text{O}_2 (g) \rightarrow \text{CO}_2 (g) \) | \(-393.6\) |
| \( \text{S} (s) + \text{O}_2 (g) \rightarrow \text{SO}_2 (g) \) | \(-296.8\) |
| \( \text{C} (s) + 2\text{S} (s) \rightarrow \text{CS}_2 (\ell) \) | \(+87.9\) |
---
**Explanation:**
- The table lists three reactions and their associated enthalpy changes, \( \Delta H \).
- The first reaction involves carbon reacting with oxygen to form carbon dioxide, releasing \(393.6 \, \text{kJ/mol}\).
- The second reaction involves sulfur reacting with oxygen to form sulfur dioxide, releasing \(296.8 \, \text{kJ/mol}\).
- The third reaction shows the formation of carbon disulfide from its elements, with an associated enthalpy change of \(+87.9 \, \text{kJ/mol}\).
**Instructions:**
To find the enthalpy change for the combustion of CS₂, apply Hess's Law, which involves manipulating the given reactions to derive the target reaction, ensuring the \( \Delta H \) values align correctly.
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