The heat of combustion of isopropyl alcohol is -2006 kJ/mol. Given the following information, calculate the heat of formation of isopropyl alcohol. AH°¢(CO,(g)) = -393-5 kJ/mol AH°; (H,0(1)) = -285.8 kJ/mol
The heat of combustion of isopropyl alcohol is -2006 kJ/mol. Given the following information, calculate the heat of formation of isopropyl alcohol. AH°¢(CO,(g)) = -393-5 kJ/mol AH°; (H,0(1)) = -285.8 kJ/mol
Chemistry
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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
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![The combustion reaction of isopropyl alcohol is:
\[ \text{C}_3\text{H}_7\text{OH}(l) + \frac{9}{2} \text{O}_2(g) \rightarrow 3 \text{CO}_2(g) + 4 \text{H}_2\text{O}(l) \]
This equation represents the chemical reaction where isopropyl alcohol (C₃H₇OH) reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). The reaction is balanced, showing the conservation of mass, where three molecules of carbon dioxide and four molecules of water are produced. This type of reaction is exothermic, releasing energy in the form of heat.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3cca2f6-99a8-4436-ac34-ddd5c6eac033%2Fdfd45b55-42f0-40e1-a4d3-5ebec6354994%2F1crs66_processed.png&w=3840&q=75)
Transcribed Image Text:The combustion reaction of isopropyl alcohol is:
\[ \text{C}_3\text{H}_7\text{OH}(l) + \frac{9}{2} \text{O}_2(g) \rightarrow 3 \text{CO}_2(g) + 4 \text{H}_2\text{O}(l) \]
This equation represents the chemical reaction where isopropyl alcohol (C₃H₇OH) reacts with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). The reaction is balanced, showing the conservation of mass, where three molecules of carbon dioxide and four molecules of water are produced. This type of reaction is exothermic, releasing energy in the form of heat.
![The heat of combustion of isopropyl alcohol is -2006 kJ/mol. Given the following information, calculate the heat of formation of isopropyl alcohol.
\(\Delta H_f^\circ (\text{CO}_2(g)) = -393.5 \, \text{kJ/mol}\)
\(\Delta H_f^\circ (\text{H}_2\text{O}(l)) = -285.8 \, \text{kJ/mol}\)
[Enter calculated value] kJ/mol
---
This text is set within a box typical of an educational problem statement, possibly for a chemistry or thermodynamics lesson. The problem provides known values for the standard enthalpy of formation of carbon dioxide and water, and asks for the calculation of the enthalpy of formation of isopropyl alcohol using the given heat of combustion. The box for entering the answer indicates it might be an interactive problem, inviting direct student input.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3cca2f6-99a8-4436-ac34-ddd5c6eac033%2Fdfd45b55-42f0-40e1-a4d3-5ebec6354994%2Fcyk5a9p_processed.png&w=3840&q=75)
Transcribed Image Text:The heat of combustion of isopropyl alcohol is -2006 kJ/mol. Given the following information, calculate the heat of formation of isopropyl alcohol.
\(\Delta H_f^\circ (\text{CO}_2(g)) = -393.5 \, \text{kJ/mol}\)
\(\Delta H_f^\circ (\text{H}_2\text{O}(l)) = -285.8 \, \text{kJ/mol}\)
[Enter calculated value] kJ/mol
---
This text is set within a box typical of an educational problem statement, possibly for a chemistry or thermodynamics lesson. The problem provides known values for the standard enthalpy of formation of carbon dioxide and water, and asks for the calculation of the enthalpy of formation of isopropyl alcohol using the given heat of combustion. The box for entering the answer indicates it might be an interactive problem, inviting direct student input.
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