3. Fig. 3-1 shows z as function of mole fraction of butane in a nitrogen/butane mixture. The figure shows line for various pressures. Explain why z for pure butane behaves so differently from z for pure nitrogen as P increases, in particular, why is the butane z non-monotonic in pressure.
3. Fig. 3-1 shows z as function of mole fraction of butane in a nitrogen/butane mixture. The figure shows line for various pressures. Explain why z for pure butane behaves so differently from z for pure nitrogen as P increases, in particular, why is the butane z non-monotonic in pressure.
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:2.0
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1.8-
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1.6-
690 bar
621
1.5는
552
1.4
483
1.3
414
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1.0
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MOLE FRACTION BUTANE
Figure 3-1
(Evans and Watson, 1956).
Compressibility factors for nitrogen/butane mixtures at 171°C
z = Pv/RT
55.2
Transcribed Image Text:3. Fig. 3-1 shows z as function of mole fraction of butane in a
nitrogen/butane mixture. The figure shows line for various
pressures. Explain why z for pure butane behaves so
differently from z for pure nitrogen as P increases, in
particular, why is the butane z non-monotonic in pressure.
Expert Solution
Step 1
Compressability factor is the measure of deviation from ideality or ideal behavior of the real gases and it is written as
Where Z is the compressability factor
P is the pressure and T is temperature
V is the volume
n is number of mole of the real gases
R is the gas constant.
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