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+//Chemical Engineering Thermodynamics

+//Chapter 2

+//P-V-T Relations

+

+//Example 2.6

+clear;

+clc;

+

+//Given

+P1 = 266;

+T1 = 473.16;//Initial temperature in Kelvin

+T2 = 273.16;//Final temperature in Kelvin

+V1 = 80; V2 = 80;//Initial & final volume in litres

+N1 = (14.28/28); N2 = (14.28/28);//Initial and final Kg moles are equal

+Tc = 126;//Critical temperature of N2 in K

+Pc = 33.5;//Critical pressure of N2 in atm

+

+//To calculate the final pressure achieved

+//(i)Using ideal gas law

+p2 = (P1*V1*N2*T2)/(V2*N1*T1);

+mprintf('(i)Final pressure of N2  using ideal gas law is %f atm',p2);

+

+//(ii)Using generalized Z chart

+Tr1 = T1/Tc;//reduced initial temp in k

+Pr1 = P1/Pc;//reduced initial press in K

+//From the Z-chart compressibility factor coressponding to the above Tr1 &Pr1 is

+Z1 = 1.07;

+P2 = [125,135,150];

+Z2 = [0.95, 0.96, 0.98];

+F = [0,0,0];

+for i = 1:3

+    F(i) = (P2(i)/(Z2(i)*T2))-(P1/(Z1*T1));

+end

+clf;

+plot(P2,F);

+xtitle("P2 vs F","P2","F");

+P3 = interpln([F;P2],0);

+mprintf('\n (ii)Final pressure of N2 from Z chart is %f atm',P3);

+

+//(iii)Using Pseudo reduced density chart

+R = 0.082;//gas constant

+v = V1/N1;//Volume per moles of nitrogen in m^3/Kg mole

+Dr = (R*Tc)/(Pc*v);

+Tr2 = T2/Tc;//final reduced temp in K

+//From figure A.2.1, reduced pressure coressponding to this Dr and Tr2 is

+Pr2 = 4.1//final reduced pressure in atm

+p2_ = Pr2*Pc;

+mprintf('\n (iii)Final pressure achieved using Dr chart is %f atm',p2_);

+//end
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