(a) Derive the equation of state, the entropy, and the internal energy of the gas. (b) Suppose that 100 moles of the gas expands from 2 m3 to 5 m³ at 280 K and that the constants have the values a = 0.364 J m³ mol-2, b = 4.27 × 10-5 m³ mol-1, and $ = 1.09 × 10-5 m³ K³/2 mol-1. Calculate: (i) AU. (ii) the maximum energy that can be made available for work due to the process.
(a) Derive the equation of state, the entropy, and the internal energy of the gas. (b) Suppose that 100 moles of the gas expands from 2 m3 to 5 m³ at 280 K and that the constants have the values a = 0.364 J m³ mol-2, b = 4.27 × 10-5 m³ mol-1, and $ = 1.09 × 10-5 m³ K³/2 mol-1. Calculate: (i) AU. (ii) the maximum energy that can be made available for work due to the process.
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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Transcribed Image Text:1. The Helmholtz function of a certain gas is given by
(V –
F (T,V) = –nRT |1+ ln
v – nb)T?
an?
пф
V
where n is the number of moles of gas, T is the temperatures of the gas, V is the volume of
the gas, and a, b, and o are constants.
(a) Derive the equation of state, the entropy, and the internal energy of the gas.
(b) Suppose that 100 moles of the gas expands from 2 m3 to 5 m³ at 280 K and that the
constants have the values a = 0.364 J m3 mol-2, b = 4.27 × 10-5 m³ mol-1, and
$ = 1.09 × 10-5 m³ K³/2 mol-1. Calculate:
(i) AU.
(ii) the maximum energy that can be made available for work due to the process.
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