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12-a. Use standard heats of formation to determine the heat of combustion for the following reaction. Heat of formation of CO₂(g) is -393.5, H₂O(g) is -241.8, and C₂H5OH is -277.6 J/mol 2C₂H5OH(1) +30₂(g) →→ 6H₂O(g) + 4CO₂(g) b. Calculate the amount of energy released from combusting 100 g of ethanol.

12-a. Use standard heats of formation to determine the heat of combustion for the following reaction. Heat of formation of CO₂(g) is -393.5, H₂O(g) is -241.8, and C₂H5OH is -277.6 J/mol 2C₂H5OH(1) +30₂(g) →→ 6H₂O(g) + 4CO₂(g) b. Calculate the amount of energy released from combusting 100 g of ethanol.

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter15: Energy And Chemical Change
Section: Chapter Questions
Problem 92A
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12- a. Use standard heats of formation to determine the heat of combustion for the following reaction. Heat of formation of CO₂(g) is -393.5, H₂O(g) is -241.8, and C₂H5OH is -277.6 J/mol 2C₂H5OH(1) + 30₂(g) → 6H₂O(g) + 4CO₂(g) b. Calculate the amount of energy released from combusting 100 g of ethanol.
Transcribed Image Text:12- a. Use standard heats of formation to determine the heat of combustion for the following reaction. Heat of formation of CO₂(g) is -393.5, H₂O(g) is -241.8, and C₂H5OH is -277.6 J/mol 2C₂H5OH(1) + 30₂(g) → 6H₂O(g) + 4CO₂(g) b. Calculate the amount of energy released from combusting 100 g of ethanol.
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