Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Thermochemical Equations for Formation of Butanol
This image presents five different balanced chemical equations, labeled A through E, all involving the formation or combustion of butanol (\(C_4H_9OH\)). Each equation includes the standard enthalpy change of formation (\(\Delta H_f^\circ\)) noted as \(-327.0 \, \text{kJ/mol}\).
**A.**
\[ 4 \, \text{C(s, graphite)} + 10 \, \text{H(g)} + \text{O(g)} \rightarrow \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**B.**
\[ 8 \, \text{C(s, graphite)} + 10 \, \text{H}_2\text{(g)} + \text{O}_2\text{(g)} \rightarrow 2 \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**C.**
\[ \text{C}_4\text{H}_9\text{OH(l)} + 6 \, \text{O}_2\text{(g)} \rightarrow 4 \, \text{CO}_2\text{(g)} + 5 \, \text{H}_2\text{O(g)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**D.**
\[ 4 \, \text{C(s, graphite)} + 5 \, \text{H}_2\text{(g)} + \frac{1}{2} \, \text{O}_2\text{(g)} \rightarrow \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**E.**
\[ 2 \, \text{C}_2\text{(s, graphite)} + 5 \, \text{H}_2\text{(g](https://content.bartleby.com/qna-images/question/b3cca2f6-99a8-4436-ac34-ddd5c6eac033/3d1f4efa-374b-4a08-86d6-4924fe61c31a/if37mw66_processed.png)
Transcribed Image Text:### Thermochemical Equations for Formation of Butanol
This image presents five different balanced chemical equations, labeled A through E, all involving the formation or combustion of butanol (\(C_4H_9OH\)). Each equation includes the standard enthalpy change of formation (\(\Delta H_f^\circ\)) noted as \(-327.0 \, \text{kJ/mol}\).
**A.**
\[ 4 \, \text{C(s, graphite)} + 10 \, \text{H(g)} + \text{O(g)} \rightarrow \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**B.**
\[ 8 \, \text{C(s, graphite)} + 10 \, \text{H}_2\text{(g)} + \text{O}_2\text{(g)} \rightarrow 2 \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**C.**
\[ \text{C}_4\text{H}_9\text{OH(l)} + 6 \, \text{O}_2\text{(g)} \rightarrow 4 \, \text{CO}_2\text{(g)} + 5 \, \text{H}_2\text{O(g)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**D.**
\[ 4 \, \text{C(s, graphite)} + 5 \, \text{H}_2\text{(g)} + \frac{1}{2} \, \text{O}_2\text{(g)} \rightarrow \text{C}_4\text{H}_9\text{OH(l)} \]
\[ \Delta H_f^\circ = -327.0 \, \text{kJ/mol} \]
**E.**
\[ 2 \, \text{C}_2\text{(s, graphite)} + 5 \, \text{H}_2\text{(g
Transcribed Image Text:The heat of formation at 25°C of liquid butanol, C₄H₉OH(l) is -327.0 kJ/mol. Which of the following is the correct heat of formation reaction for C₄H₉OH(l)?
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