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One mole of hydrogen and one mole of air (80% N2 and 20% O2) are mixed at 298 K and burned under adiabatic and constant pressure condition. Calculate the adiabatic flame temperature. 3. i. AHH20, 298K = -246,000 J/mol ii. CP, H20 (9) = 30.00 J/K.mol iv. CP, N2 = 20.79 J/K.mol Data: iii. CP, H2 = 27.37 J/K.mol v. CP, 02 = 29.96 J/K.mol (Note that all data may not be required.) 8.

One mole of hydrogen and one mole of air (80% N2 and 20% O2) are mixed at 298 K and burned under adiabatic and constant pressure condition. Calculate the adiabatic flame temperature. 3. i. AHH20, 298K = -246,000 J/mol ii. CP, H20 (9) = 30.00 J/K.mol iv. CP, N2 = 20.79 J/K.mol Data: iii. CP, H2 = 27.37 J/K.mol v. CP, 02 = 29.96 J/K.mol (Note that all data may not be required.) 8.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
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One mole of hydrogen and one mole of air (80% N2 and 20% 02) are mixed at 298 K and burned under adiabatic and constant pressure condition. Calculate the adiabatic flame temperature. 3. i. AHH20, 298K = -246,000 J/mol ii. CP, H20 (g) = 30.00 J/K.mol iv. CP, N2 = 20.79 J/K.mol Data: iii. CP, H2 = 27.37 J/K.mol v. CP, 02 = 29.96 J/K.mol (Note that all data may not be required.) 8
Transcribed Image Text:One mole of hydrogen and one mole of air (80% N2 and 20% 02) are mixed at 298 K and burned under adiabatic and constant pressure condition. Calculate the adiabatic flame temperature. 3. i. AHH20, 298K = -246,000 J/mol ii. CP, H20 (g) = 30.00 J/K.mol iv. CP, N2 = 20.79 J/K.mol Data: iii. CP, H2 = 27.37 J/K.mol v. CP, 02 = 29.96 J/K.mol (Note that all data may not be required.) 8
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