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

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

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

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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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