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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
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