From b1f5c3f8d6671b4331cef1dcebdf63b7a43a3a2b Mon Sep 17 00:00:00 2001
From: priyanka
Date: Wed, 24 Jun 2015 15:03:17 +0530
Subject: initial commit / add all books

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 479/CH2/EX2.7/Example_2_7.sce | 31 +++++++++++++++++++++++++++++++
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diff --git a/479/CH2/EX2.7/Example_2_7.sce b/479/CH2/EX2.7/Example_2_7.sce
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+//Chemical Engineering Thermodynamics
+//Chapter 2
+//P-V-T Relations
+
+//Example 2.7
+clear;
+clc;
+
+//Given
+n = 1;//n is the Kg mole of methane gas
+T = 298;//T is the constant temperature in K
+P1 = 1;//P1 is the initial pressure of the system
+P2 = 100;//P2 is the final pressure of the system
+R = 8314.4;//R is the gas constant in Nm/Kgmole deg K
+
+//To compute the work required
+//(i)Using ideal gas law
+W = R*T*log(P1/P2);
+mprintf('(i)Work done by the system if the gas obeys ideal gas law is %4.2e Nm',W);
+
+//(ii)Using Vander Waals' equation
+//Given
+//For methane
+a = 2.32*(10^5);//Vander Wals' constant a in N/m^2
+b = 0.0428;//Vanderwaals' constant b in m^3
+//V1 and V2 are evaluated by trial and error using Vanderwaals' equation as P1 and P2 are known
+V1 = 11.1;//initial volume of the gas in m^3
+V2 = 0.089;//final volume of the gas in m^3
+W = (R*T*log((V2-b)/(V1-b)))+(a*((1/V2)-(1/V1)))
+mprintf('\n (ii)Work done by the system if the gas obeys Vander Waals equation is %4.2e Nm',W);
+//end
\ No newline at end of file
-- 
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