a) 1 mol of liquid ethanol is at 25 ºC, and has been adiabatically compressed from 1 atm to 20 atm. Assuming ethanol is incompressible, calculate U and H. �(ethanol)= 0.789 g/mL.
a) 1 mol of liquid ethanol is at 25 ºC, and has been adiabatically compressed from 1 atm to 20 atm. Assuming ethanol is incompressible, calculate U and H. �(ethanol)= 0.789 g/mL.
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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a) 1 mol of liquid ethanol is at 25 ºC, and has been adiabatically
compressed from 1 atm to 20 atm. Assuming ethanol is
incompressible, calculate U and H. �(ethanol)= 0.789 g/mL.
b) When 0.15 g of a substance are burned at constant V, the
temperature rises to 6.568 K. Calculate the standard combustion
enthalpy of the substance assuming ΔU≃ΔH. If in this reaction
Δn≃1, discuss if such an assumption is acceptable or not.
Data: q = k*ΔT ; T = 298 K; molecular weight of the substance: 132
g/mol; k = 715 J/K.
Transcribed Image Text:compressed from 1 atm to 20 atm. Assuming ethanol is
incompressible, calculate U and H. p(ethanol)= 0.789 g/mL.
b) When 0.15 g of a substance are burned at constant V, the
temperature rises to 6.568 K. Calculate the standard combustion
enthalpy of the substance assuming AU=AH. If in this reaction
An=1, discuss if such an assumption is acceptable or not.
Data: q = k*AT ;T = 298 K; molecular weight of the substance: 132
g/mol; k = 715 J/K.
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