Hydrazine, N2H4, is a liquid substance used in rocket fuels. Its combustion liberates 622.4 kJ of energy. For the reaction: N2H4(l) + O2(g) → N2(g) + 2 H2O (l) ∆H°rxn = -622.4 kJ a. Calculate the ∆Hf of hydrazine. b. The absolute entropy of hydrazine is 219.5 J/ K•mol, Use the standard thermodynamics value to calculate the ∆S° for the reaction. c. Use the standard enthalpy and entropy of the reaction to calculate the ∆G°. d. Use the values of ∆G° for the reaction to calculate the Gibb’s free energy of formation of hydrazine.
Hydrazine, N2H4, is a liquid substance used in rocket fuels. Its combustion liberates 622.4 kJ of energy. For the reaction: N2H4(l) + O2(g) → N2(g) + 2 H2O (l) ∆H°rxn = -622.4 kJ a. Calculate the ∆Hf of hydrazine. b. The absolute entropy of hydrazine is 219.5 J/ K•mol, Use the standard thermodynamics value to calculate the ∆S° for the reaction. c. Use the standard enthalpy and entropy of the reaction to calculate the ∆G°. d. Use the values of ∆G° for the reaction to calculate the Gibb’s free energy of formation of hydrazine.
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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Hydrazine, N2H4, is a liquid substance used in rocket fuels. Its combustion liberates 622.4 kJ of
energy. For the reaction: N2H4(l) + O2(g) → N2(g) + 2 H2O (l) ∆H°rxn = -622.4 kJ
a. Calculate the ∆Hf of hydrazine.
b. The absolute entropy of hydrazine is 219.5 J/ K•mol, Use the standard
to calculate the ∆S° for the reaction.
c. Use the standard enthalpy and entropy of the reaction to calculate the ∆G°.
d. Use the values of ∆G° for the reaction to calculate the Gibb’s free energy of formation of
hydrazine.
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