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Calculate the enthalpy of the reaction: H2,(g) + ¹/2O2, (g) → H₂O(g) at 350°C, in kJ/mole. Note: Assume that reactants enter at 350°C and products exit at 350°C. Your Answer: Answer

Calculate the enthalpy of the reaction: H2,(g) + ¹/2O2, (g) → H₂O(g) at 350°C, in kJ/mole. Note: Assume that reactants enter at 350°C and products exit at 350°C. Your Answer: Answer

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
Problem 1.1P
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Calculate the enthalpy of the reaction: H2,(g) + 1/2O2, (g) → H₂O(g) at 350°C, in kJ/mole. Note: Assume that reactants enter at 350°C and products exit at 350°C. Your Answer: Answer Hide hint for Question 6 • Use values from B.1 and B.8 • If your answer was wrong and you are trying to reverse engineer the answer, take notice of the fact that the "correct" answer might be slightly off as it uses interpolation over a wide range of temperatures.
Transcribed Image Text:Calculate the enthalpy of the reaction: H2,(g) + 1/2O2, (g) → H₂O(g) at 350°C, in kJ/mole. Note: Assume that reactants enter at 350°C and products exit at 350°C. Your Answer: Answer Hide hint for Question 6 • Use values from B.1 and B.8 • If your answer was wrong and you are trying to reverse engineer the answer, take notice of the fact that the "correct" answer might be slightly off as it uses interpolation over a wide range of temperatures.
table B.1 SG Compound Formula Mol. Wt. (20°/4°) Tm(°C)b Hydrogen H₂ 2.016 -259.19 Oxygen 0₂ AĤm(Tm).j 32.00 T -218.75 kJ/mol Tb (°C)d -252.76 0.12 0.444 -182.97 AĤv(Tb).j kJ/mol T.(K) P.(atm) 0.904 33.3 12.8 6.82 Table B.8 Specific Enthalpies of Selected Gases: SI Units Ĥ (kJ/mol) Reference state: Gas, Pref= 1 atm, Tref = 25°C Air 0₂ N₂ H₂ CO CO₂ 0 -0.72 -0.73 -0.73 -0.72 -0.73 -0.92 25 0.00 0.00 0.00 0.00 0.00 0.00 100 2.19 2.24 2.19 2.16 2.19 2.90 200 5.15 5.31 5.13 5.06 5.16 7.08 300 8.17 8.47 8.12 7.96 8.17 11.58 400 11.24 11.72 11.15 10.89 11.25 16.35 500 14.37 15.03 14.24 13.83 14.38 21.34 600 17.55 18.41 17.39 16.81 17.57 26.53 700 20.80 21.86 20.59 19.81 20.82 31.88 800 24.10 25.35 23.86 22.85 24.13 37.36 900 27.46 28.89 27.19 25.93 27.49 42.94 1000 30.86 32.47 30.56 29.04 30.91 48.60 1100 34.31 36.07 33.99 32.19 34.37 54.33 1200 37.81 39.70 37.46 35.39 37.87 60.14 1300 41.34 43.38 40.97 38.62 41.40 65.98 41.90 44.95 71.89 1400 44.89 47.07 44.51 1500 48.45 50.77 48.06 45.22 48.51 77.84 154.4 H₂O -0.84 0.00 2.54 6.01 9.57 13.23 17.01 20.91 24.92 29.05 33.32 37.69 42.18 46.78 51.47 56.25 61.09 49.7 (AĤ°) ¹.j kJ/mol 0(g) 0(g) (ΔΗ °). kJ/mol -285.84(g)
Transcribed Image Text:table B.1 SG Compound Formula Mol. Wt. (20°/4°) Tm(°C)b Hydrogen H₂ 2.016 -259.19 Oxygen 0₂ AĤm(Tm).j 32.00 T -218.75 kJ/mol Tb (°C)d -252.76 0.12 0.444 -182.97 AĤv(Tb).j kJ/mol T.(K) P.(atm) 0.904 33.3 12.8 6.82 Table B.8 Specific Enthalpies of Selected Gases: SI Units Ĥ (kJ/mol) Reference state: Gas, Pref= 1 atm, Tref = 25°C Air 0₂ N₂ H₂ CO CO₂ 0 -0.72 -0.73 -0.73 -0.72 -0.73 -0.92 25 0.00 0.00 0.00 0.00 0.00 0.00 100 2.19 2.24 2.19 2.16 2.19 2.90 200 5.15 5.31 5.13 5.06 5.16 7.08 300 8.17 8.47 8.12 7.96 8.17 11.58 400 11.24 11.72 11.15 10.89 11.25 16.35 500 14.37 15.03 14.24 13.83 14.38 21.34 600 17.55 18.41 17.39 16.81 17.57 26.53 700 20.80 21.86 20.59 19.81 20.82 31.88 800 24.10 25.35 23.86 22.85 24.13 37.36 900 27.46 28.89 27.19 25.93 27.49 42.94 1000 30.86 32.47 30.56 29.04 30.91 48.60 1100 34.31 36.07 33.99 32.19 34.37 54.33 1200 37.81 39.70 37.46 35.39 37.87 60.14 1300 41.34 43.38 40.97 38.62 41.40 65.98 41.90 44.95 71.89 1400 44.89 47.07 44.51 1500 48.45 50.77 48.06 45.22 48.51 77.84 154.4 H₂O -0.84 0.00 2.54 6.01 9.57 13.23 17.01 20.91 24.92 29.05 33.32 37.69 42.18 46.78 51.47 56.25 61.09 49.7 (AĤ°) ¹.j kJ/mol 0(g) 0(g) (ΔΗ °). kJ/mol -285.84(g)
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