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+
+// Theory and Problems of Thermodynamics
+// Chapter 5
+//Second Law of Thermodynamcis
+// Example 15
+
+clear ;clc;
+
+//Given data
+N1 = 2          // number of moles of helium
+P1 = 1.0*1e6    // pressure of helium compartment in Pa
+T1 = 600        // temperature of helium compartment in K
+N2 = 5          // number of moles of air
+P2 = 2.0*1e6    // pressure of air compartment in Pa
+T2 = 500        // temperature of air compartment in K
+R = 8.314       // universal gas constant J/mol/K
+C1 = 1.5 * R    // specific heat(ischoric) of helium in kJ/kmol/K
+C2 = 2.5 * R    // specific heat(ischoric) of air in kJ/kmol/K
+
+// Calculations for determining the entorphy change of given process
+V1 = N1*T1*R/P1     // volume of helium before mixing
+V2 = N2*T2*R/P2     // volume of air    before mixing
+
+// Consider the entire container as the system, then Q = 0; W = 0;
+// Hence, del U = 0; 
+deff('y=Tf(T)', 'y = N1*C1*(T-T1) + N2*C2*(T-T2)')
+T = fsolve(0,Tf)    // Final temperature after mixing
+
+V = V1 + V2         // final volume   after mixing
+N = N1 + N2         // total moles    after mixing
+P = N*T*R/V         // Final pressure after mixing in Pa
+
+// entropy change for helium from initial state to final state
+S1 = N1*{2.5*R*log(T/T1) - R*log(P/P1)}
+
+// entropy change for air from initial state to final state
+S2 = N2*{3.5*R*log(T/T2) - R*log(P/P2)}
+
+// entropy change for final state of individual to mixture
+S3 = -7*R*{(N1/N)*log(N1/N) + (N2/N)*log(N2/N)}
+
+// The Total change in enthalphy for entire process 
+S = S1 + S2 + S3
+
+// Output Results
+mprintf('The entrophy change for associated with the process = %6.4f kJ/K' ,S)
+