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 --- 479/CH13/EX13.1/Example_13_1.sce | 30 ++++++++++++++++++++++ 479/CH13/EX13.10/Exampe_13_10.sce | 11 ++++++++ 479/CH13/EX13.11/Example_13_11.sce | 11 ++++++++ 479/CH13/EX13.12/Example_13_12.sce | 31 +++++++++++++++++++++++ 479/CH13/EX13.13/Example_13_13.sce | 43 +++++++++++++++++++++++++++++++ 479/CH13/EX13.14/Example_13_14.sce | 28 ++++++++++++++++++++ 479/CH13/EX13.15/Example_13_15.sce | 30 ++++++++++++++++++++++ 479/CH13/EX13.16/Example_13_16.sce | 48 +++++++++++++++++++++++++++++++++++ 479/CH13/EX13.17/Example_13_17.sce | 40 +++++++++++++++++++++++++++++ 479/CH13/EX13.17/Example_13_17.txt | 3 +++ 479/CH13/EX13.18/Example_13_18.sce | 33 ++++++++++++++++++++++++ 479/CH13/EX13.19/Example_13_19.sce | 36 ++++++++++++++++++++++++++ 479/CH13/EX13.19/Example_13_19.txt | 4 +++ 479/CH13/EX13.2/Example_13_2.sce | 22 ++++++++++++++++ 479/CH13/EX13.3/Example_13_3.sce | 27 ++++++++++++++++++++ 479/CH13/EX13.4/Example_13_4.sce | 37 +++++++++++++++++++++++++++ 479/CH13/EX13.5/Example_13_5.sce | 11 ++++++++ 479/CH13/EX13.6/Example_13_6.sce | 24 ++++++++++++++++++ 479/CH13/EX13.7/Example_13_7.sce | 52 ++++++++++++++++++++++++++++++++++++++ 479/CH13/EX13.8/Example_13_8.sce | 26 +++++++++++++++++++ 479/CH13/EX13.9/Example_13_9.sce | 11 ++++++++ 21 files changed, 558 insertions(+) create mode 100755 479/CH13/EX13.1/Example_13_1.sce create mode 100755 479/CH13/EX13.10/Exampe_13_10.sce create mode 100755 479/CH13/EX13.11/Example_13_11.sce create mode 100755 479/CH13/EX13.12/Example_13_12.sce create mode 100755 479/CH13/EX13.13/Example_13_13.sce create mode 100755 479/CH13/EX13.14/Example_13_14.sce create mode 100755 479/CH13/EX13.15/Example_13_15.sce create mode 100755 479/CH13/EX13.16/Example_13_16.sce create mode 100755 479/CH13/EX13.17/Example_13_17.sce create mode 100755 479/CH13/EX13.17/Example_13_17.txt create mode 100755 479/CH13/EX13.18/Example_13_18.sce create mode 100755 479/CH13/EX13.19/Example_13_19.sce create mode 100755 479/CH13/EX13.19/Example_13_19.txt create mode 100755 479/CH13/EX13.2/Example_13_2.sce create mode 100755 479/CH13/EX13.3/Example_13_3.sce create mode 100755 479/CH13/EX13.4/Example_13_4.sce create mode 100755 479/CH13/EX13.5/Example_13_5.sce create mode 100755 479/CH13/EX13.6/Example_13_6.sce create mode 100755 479/CH13/EX13.7/Example_13_7.sce create mode 100755 479/CH13/EX13.8/Example_13_8.sce create mode 100755 479/CH13/EX13.9/Example_13_9.sce (limited to '479/CH13') diff --git a/479/CH13/EX13.1/Example_13_1.sce b/479/CH13/EX13.1/Example_13_1.sce new file mode 100755 index 000000000..5f1481c3f --- /dev/null +++ b/479/CH13/EX13.1/Example_13_1.sce @@ -0,0 +1,30 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.1 +clear; +clc; + +//Given +//N2 obeys the relation : Z = 1+(2.11*10^-4*P) +Tc = 126;//Critical temperature in K +Pc = 33.5;//Critical pressure in atm +T = 373;//in K +P = 100;//in atm + +//To Calculate the fugacity of N2 at 373K and 100 atm +//(i)Using the Z relation given above +//From equation 13.12 (page no 239) +phi = %e^(2.11*10^-4*(P-0));//fugacity coefficient +f = phi*P; +mprintf('(i)The fugacity of N2 using the given Z relation is %f atm',f); + +//(ii)Using the fugacity chart given in figure A.2.9 +Pr = P/Pc;//Reduced pressure in atm +Tr = T/Tc;//Reduced temperature in K +//From figure A.2.9, +phi = 1.04 +f = phi*P; +mprintf('\n (ii)The fugacity of N2 using the fugacity chart is %f atm',f); +//end \ No newline at end of file diff --git a/479/CH13/EX13.10/Exampe_13_10.sce b/479/CH13/EX13.10/Exampe_13_10.sce new file mode 100755 index 000000000..e6a74d9ba --- /dev/null +++ b/479/CH13/EX13.10/Exampe_13_10.sce @@ -0,0 +1,11 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.10 +clear; +clc; + +//Given +//The given example is a theoretical problem and does not involve any numerical computation +//end \ No newline at end of file diff --git a/479/CH13/EX13.11/Example_13_11.sce b/479/CH13/EX13.11/Example_13_11.sce new file mode 100755 index 000000000..dbd0fb26e --- /dev/null +++ b/479/CH13/EX13.11/Example_13_11.sce @@ -0,0 +1,11 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.11 +clear; +clc; + +//Given +//The given example is a theoretical problem and does not involve any numerical computation +//end \ No newline at end of file diff --git a/479/CH13/EX13.12/Example_13_12.sce b/479/CH13/EX13.12/Example_13_12.sce new file mode 100755 index 000000000..c31b3fdf3 --- /dev/null +++ b/479/CH13/EX13.12/Example_13_12.sce @@ -0,0 +1,31 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.12 +clear; +clc; + +//Given +x_A = [0 0.0435 0.0942 0.1711 0.2403 0.3380 0.5981];//mole fraction of acetic acid +p_A = [0 17.2 30.5 46.5 57.8 69.3 95.7];//partial pressure of acetic acid in mmHg +P_T1 = 202;//vapour pressure of toulene in mmHg +P_T2_ex = 167.3;//experimental partial pressure in mmmHg + +//To Calculate the partial pressure of toulene in the solution and check with the experimental value +//From the equation 13.95, +//ln(P_T2/P_T1) = -intg(x_A/((1-x_A)*p_A)) +for i = 1:7 + if (p_A(i) ~= 0) + x(i) = (x_A(i)/((1-x_A(i))*p_A(i)))*10^4 + end +end +plot(x,p_A); +xtitle(" ","(x_A/((1-x_A)*p_A))*10^4", "p_A"); +//Area of the graph drawn is +A = -0.138; +P_T2 = (%e^A)*P_T1; +e = ((P_T2-P_T2_ex)*100)/P_T2_ex; +mprintf('The partial pressure of toulene is %f mmHg',P_T2); +mprintf('\n This deviates %i percent from the reported value',e); +//end \ No newline at end of file diff --git a/479/CH13/EX13.13/Example_13_13.sce b/479/CH13/EX13.13/Example_13_13.sce new file mode 100755 index 000000000..8360364b0 --- /dev/null +++ b/479/CH13/EX13.13/Example_13_13.sce @@ -0,0 +1,43 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.13 +clear; +clc; + +//Given +P = 760;//pressure at maximum boiling azeotrope of A and B in mmHg +x_A = 0.6;//mole fraction of A in liquid phase +x_B = 0.4;//mole fraction of B in liquid phase +p_A = 600;//vapour pressure of A at 90 deg cel +p_B = 300;//vapour pressure of B at 90 deg cel + +//To Check whether the activity coefficient of the solution can be represented by the Margules equation +y_A = P/p_A;//Activity coefficient of A +y_B = P/p_B;//Activity coefficient of B +//From the Margules equation or equation (a) & (b) +U = [((x_B^2)-(2*(x_B^2)*x_A)) (2*(x_B^2)*x_A); (2*(x_A^2)*x_B) ((x_A^2)-(2*(x_A^2)*x_B))]; +V = [log(y_A); log(y_B)]; +W = U\V; +//Now the value of constants A and B in equations(a)&(b) are given as +A = W(1); +B = W(2); +//let us assume +x_A = [0.0 0.2 0.4 0.6 0.8 1.0]; +x_B = [1.0 0.8 0.6 0.4 0.2 0.0]; +//C = lny_A; D = lny_B; E = ln(y_A/y_B) +for i = 1:6 + C(i) = (x_B(i)^2)*(2*(B-A)*x_A(i)+A); + D(i) = (x_A(i)^2)*(2*(A-B)*x_B(i)+B); + E(i) = C(i)-D(i); +end +clf; +plot(x_A,E); +xtitle(" ","x_A","ln(y_A/y_B)"); +a = get("current_axes"); +set(a,"x_location","origin"); +//Since the graph drawn is approximately symmetrical.Thus it satisfies the Redlich-Kister Test +mprintf('The actvity coefficients of the system can be represented by Margules equation'); +//end + diff --git a/479/CH13/EX13.14/Example_13_14.sce b/479/CH13/EX13.14/Example_13_14.sce new file mode 100755 index 000000000..5c812b361 --- /dev/null +++ b/479/CH13/EX13.14/Example_13_14.sce @@ -0,0 +1,28 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.14 +clear; +clc; + +//Given +P = 760;//Total pressure of the mixture in mmHg +T = [80 90 95 100];//Temperature in deg celsius +P1 = [87.4 129.0 162.0 187.0];//vapour pressure of 1,1,2,2-tetrachloroethane in mmHg +P2 = [356 526 648 760];//Vapour pressure of water in mmHg + +//To Calculate the composition of the vapour evolved +clf; +plot2d(T,P1,style=3); +plot2d(T,P2,style=5); +xtitle(" ","Temp in deg cel","Vapour pressure in mmHg"); +legend("1,1,2,2-tetrachloroethane","Water"); +//From the graph we conclude that at 93.8 deg cel +P1 = 155;//in mm Hg +P2 = 605;//in mm Hg +y_1 = P1/P; +y_2 = P2/P; +mprintf('Mole fraction of 1,1,2,2-tetrachloroethane in vapour is %f',y_1); +mprintf('\n Mole fraction of water in vapour is %f',y_2); +//end \ No newline at end of file diff --git a/479/CH13/EX13.15/Example_13_15.sce b/479/CH13/EX13.15/Example_13_15.sce new file mode 100755 index 000000000..bcf443b19 --- /dev/null +++ b/479/CH13/EX13.15/Example_13_15.sce @@ -0,0 +1,30 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.15 +clear; +clc; + +//Given +T = [146.2 142.3 126.1 115.9 95.0 98.0 100];//Temperature in deg cel +P1 = [760.0 685.0 450.3 313.0];//Vapour pressure of 1,1,2,2-tetrachloroethane at the coressponding temperature in mm Hg +P2_5 = 648.0;//Vapour pressure of water at 95 deg cel in mm Hg +P2_6 = 711.0;//Vapour pressure of water at 98 deg cel in mm Hg +P = 760;//Total pressure of mixture in mm Hg + +x1 = [0 0 0 0 0 0 0]; +//To plot a graph between temperature and vapour phase composition +for i = 1:4 + x1(i) = P1(i)/P;//mole fraction of 1,1,2,2-tetrachloroethane +end +x2_5 = P2_5/P;//mole fraction of water at 95 deg cel +x2_6 = P2_6/P;//mole fraction of water at 98 deg cel +x1(5) = 1-x2_5; +x1(6) = 1-x2_6; + +clf; +plot(x1,T); +xtitle("","mole fraction of 1,1,2,2-tetrachloroethane","Temperature in deg cel"); +mprintf('The required graph has been ploted in the graphic window'); +//end \ No newline at end of file diff --git a/479/CH13/EX13.16/Example_13_16.sce b/479/CH13/EX13.16/Example_13_16.sce new file mode 100755 index 000000000..fd786013e --- /dev/null +++ b/479/CH13/EX13.16/Example_13_16.sce @@ -0,0 +1,48 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.16 +clear; +clc; + +//Given +//B = -(1.203*10^10)*(T^2.7); second virial coefficient, T is in K +//log P = 6.95464-(1344.8/(219.482+t))...(a);Vapour pressure of toulene +t = 107.2;//Temperature in deg cel +T = t+273.16;//in K +H_ex = 7964;//experimental value of heat of vapourisation in Kcal/Kgmole +d = 800;//density of liquid toulene in Kg/cubic meter +R = 1.98;//gas constant in Kcal/Kgmole K +M = 92.14;//molecular weight of toulene + +//To Calculate the heat of vapourization of toulene by using ideal gas law, second virial coefficient but neglecting vl and including vl +//From equation (a), let K = dlogP/dT +K = 1344.8/(219.482+t)^2; +//(i)Using ideal gas behaviour +//From equation 13.112(page no 286) +H_c = (2.303*R*(T^2))*K; +mprintf('(i)The heat of vapourization using ideal gas behaviour is %f Kcal/Kgmole',H_c); +D = ((H_c-H_ex)/H_c)*100; +mprintf('\n The deviation is %f percent',D); + +//(ii)Using second virial coeff but neglecting vl +//From equation(a) +P = 10^(6.95464-1344.8/(219.482+t));//in mm Hg +P1 = P*1.033*10^4/760;//in Kgf/sq m +B = -((1.203*10^10)/(T^2.7))*10^-3;//in cubic meter/Kgmole +//From equation 13.111 (page no 286) neglecting vl, +l = (R*T)+((B*P1)/427);//in Kcal/Kgmole +H_c = K*2.303*T*l; +mprintf('\n\n(ii)The heat of vapourisation using second virial coefficient but neglecting vl is %f Kcal/Kgmole',H_c); +D = ((H_c-H_ex)/H_c)*100; +mprintf('\n The deviation in this case is %f percent',D); + +//(iii)Using second virial coeff including vl +vl = M/d;//Liquid specific volume in cubic meter/Kgmole +n = P1*vl/427;//in Kcal/Kgmole +H_c = K*2.303*T*(l-n); +mprintf('\n\n(iii)The heat of vapourisation using second virial coefficient including vl is %f Kcal/Kgmole',H_c); +D = ((H_c-H_ex)/H_c)*100; +mprintf('\n The deviation in this case is %f',D); +//end \ No newline at end of file diff --git a/479/CH13/EX13.17/Example_13_17.sce b/479/CH13/EX13.17/Example_13_17.sce new file mode 100755 index 000000000..02cb59dac --- /dev/null +++ b/479/CH13/EX13.17/Example_13_17.sce @@ -0,0 +1,40 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.17 +clear; +clc; + +//Given +H_ex = 539;//Heat of vapoization of water in Kcal/Kg +Tc = 647;//Critical temperature in K +Pc = 218;//Critical pressure in atm +Tb = 373;//Boiling point of water in K +t = 100;//temperature in deg cel +M = 18;//Molecular weight of water +P = 1;//pressure at boiling point in atm +P1 = 1.033*10^4;//pressure in Kgf/sq m + +//To Calculate the heat of vapourisation of water by Vishwanath and Kuloor method and by Riedel's method and compare with the experimental value +//(i) Using Vishwanath and Kuloor method +H_c = (4.7*Tc*((1-(P/Pc))^0.69)*log(P/Pc))/((1-(Tc/Tb))*18); +mprintf('(i)The heat of vapourisation of water using Vishwanath and Kuloor method is %f Kcal/Kg',H_c); +D = (H_c-H_ex)*100/H_c; +mprintf('\n The deviation occurs using this method is %f percent',D); + +//(ii)Using Riedel's method +H_c = (Tb*2.17*(log(218)-1))/((0.93-(Tb/Tc))*18); +mprintf('\n\n(ii)The heat of vapourisation of water using Riedel method is %f Kcal/Kg',H_c); +D = (H_c-H_ex)*100/H_c; +mprintf('\n The deviation occurs using this method is %f percent',D); + +//(iii)By using given vapour equation; logP = 8.2157-(2218.8537/(273.16+t)), t is in deg cel +//From steam table, +Vv = 1.673;//in cubic meter/Kg +Vl = 0.001;//in cubic meter/Kg +H_c = (2218.8/(273.16+t)^2)*(2.3*Tb*P1*(Vv-Vl)/427); +mprintf('\n\n(iii)The heat of vapourisation using the given vapour equation is %f Kcal/Kg',H_c); +D = (H_c-H_ex)*100/H_c; +mprintf('\n The deviation occurs using this method is %f percent',D); +//end \ No newline at end of file diff --git a/479/CH13/EX13.17/Example_13_17.txt b/479/CH13/EX13.17/Example_13_17.txt new file mode 100755 index 000000000..59ddec64e --- /dev/null +++ b/479/CH13/EX13.17/Example_13_17.txt @@ -0,0 +1,3 @@ +For example 13.17(i), the answer given in the book, heat of vapourisation H_c = 532Kcal/Kg and the deviation as 1.3 % + but i am getting H_c = 1234.397 Kcal/Kg,using the Vishwanath and Kuloor method + and the deviation is 56.335 %.There might be some calculation mistake in the book. \ No newline at end of file diff --git a/479/CH13/EX13.18/Example_13_18.sce b/479/CH13/EX13.18/Example_13_18.sce new file mode 100755 index 000000000..748a8434e --- /dev/null +++ b/479/CH13/EX13.18/Example_13_18.sce @@ -0,0 +1,33 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.18 +clear; +clc; + +//Given +T1 = 273-87;//temp in K +T2 = 273;//temp in K +H1 = 115;//Latent heat of saturated ethane at 1 atm and -87 deg cel in Kcal/Kg +H2_ex = 72.44;//Experimental value of latent heat at 0 deg cel in Kcal/Kg +Tc = 306;//Critical temperature in K +M = 30;//Molecular weight of ethane + +//To Calculate the latent heat of saturated ethane at 0 deg cel +Tr1 = T1/Tc;//reduced temp in K +Tr2 = T2/Tc;//reduced temp in K +//(i)Using Waton's method: +H2_c = H1*((1-Tr2)/(1-Tr1))^0.38; +mprintf('(i)The latent heat of saturated ethane at 0 deg cel using Waton method is %f Kcal/Kg',H2_c); +D = (H2_ex-H2_c)*100/H2_ex; +mprintf('\n The deviation occurs using this method is %f percent',D); + +//(ii)Using Vishwanath and Kuloor method +//From equation 13.117 (page no 289) +n = (0.00133*(H1*M/T1)+0.8794)^(1/0.1); +H2_c = H1*((1-Tr2)/(1-Tr1))^n; +mprintf('\n\n(ii)The latent heat of saturated ethane at 0 deg cel using Vishwanath and Kuloor method is %f Kcal/Kg',H2_c); +D = (H2_ex-H2_c)*100/H2_ex; +mprintf('\n The deviation occurs using this method is %f percent',D); +//end \ No newline at end of file diff --git a/479/CH13/EX13.19/Example_13_19.sce b/479/CH13/EX13.19/Example_13_19.sce new file mode 100755 index 000000000..09dfa1409 --- /dev/null +++ b/479/CH13/EX13.19/Example_13_19.sce @@ -0,0 +1,36 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.19 +clear; +clc; + +//Given +H_s_ex = 32.7;//experimental value of latent heat of the solution in KJ/mole +x1 = 0.536;//mole percent of toulene in the solution +x2 = 1-0.536;//mole percent of 1,1,1-trichloroethane in the solution +H1 = 33.34;//Latent heat of toulene in KJ/gmole +H2 = 29.72;//Latent heat of 1,1,1-trichloroethane in KJ/gmole +He = 0;//excess enthalpy is neglected +Cp1 = 39.55;//Specific heat of toulene in cal/gmole deg cel +Cp2 = 24.62;//Specific heat of 1,1,1-trichloroethane in cal/gmole deg cel +T_D = 100;//dew point temperature in deg cel +T_B = 92.6;//bubble point temperature in deg cel + +//To calculate the latent heat of the solution and compare it with the one which calculated from the given vapour pressure equation +//(i)Calculation of latent heat of the solution +//From equation 13.118 (page no 291) +H_s = H1*x1+H2*x2+He+(Cp1*x1+Cp2*x2)*10^-3*4.17*(T_D-T_B); +mprintf('(i)The latent heat of the solution is %f KJ/gmole',H_s); +D = ((H_s_ex-H_s)*100)/H_s_ex; +mprintf('\n The deviation occurs using this method is %f percent',D); + +//(ii)Calculation of latent heat from the vapour pressure equation +//From equation (a) (page no 291) +K = 1657.599/((273.16+5)^2); +H_s = (K*2.303*8.314*(273.16+5)^2)*10^-3; +mprintf('\n\n(ii)The latent heat of the solution is %f KJ/gmole',H_s); +D = ((H_s_ex-H_s)*100)/H_s_ex; +mprintf('\n The deviation occurs using this method is %f percent',D); +//end \ No newline at end of file diff --git a/479/CH13/EX13.19/Example_13_19.txt b/479/CH13/EX13.19/Example_13_19.txt new file mode 100755 index 000000000..aeffb16d5 --- /dev/null +++ b/479/CH13/EX13.19/Example_13_19.txt @@ -0,0 +1,4 @@ +For example 13.19, the answer given in the book in part(i), deviation as 0.91% but i am getting deviation as 0.1%. + and for part(ii) i am getting heat of vapourization as 31.74 KJ/gmole and deviation as 2.94%. + but in the book it is given as heat of vapourization as 32.1 KJ/gmole and deviation as 1.8%. + There might be some calculation mistake in the book. \ No newline at end of file diff --git a/479/CH13/EX13.2/Example_13_2.sce b/479/CH13/EX13.2/Example_13_2.sce new file mode 100755 index 000000000..a770036e1 --- /dev/null +++ b/479/CH13/EX13.2/Example_13_2.sce @@ -0,0 +1,22 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.2 +clear; +clc; + +//Given +P1 = 50*1.03*10^4;//Initial pressure in Kgf/sq m +T = 373;//Temperature in K +P2 = 1.03*10^4;//Final pressure in Kgf/sq m +V = 0.001*18;//Volume in cubic meter +R = 848;//gas constant in m Kgf/Kgmole K + +//To Calculate the fugacity of liquid water +//From equation 13.13(page no 240) +del_u = (V/(R*T))*(P2-P1);//del_u = ln(f2/f1); Change in chemical potential +f1 = P2;//in Kgf/sq m +f2 = f1*(%e^del_u); +mprintf('The fugacity of the liquid water at 50 atm is %4.2e Kgf/sq m',f2); +//end \ No newline at end of file diff --git a/479/CH13/EX13.3/Example_13_3.sce b/479/CH13/EX13.3/Example_13_3.sce new file mode 100755 index 000000000..cfe3f9ae3 --- /dev/null +++ b/479/CH13/EX13.3/Example_13_3.sce @@ -0,0 +1,27 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.3 +clear; +clc; + +//Given +x1 = 0.1;//mole fraction of methane +x2 = 0.9;//mole fraction of propane +P = [28.1 31.6 35.1];//Pressure in Kgf/sq cm are +K1 = [5.8 5.10 4.36];//Vapourisation constants of methane at the corresponding presssures +K2 = [0.61 0.58 0.56];//Vapourisation constants of propane at the correspondig pressures + +//To Calculate the bubble point pressure of the solution +//From equation 13.27 (page no 245) +for i = 1:3 + y1(i) = K1(i)*x1;//mole fraction of methane in the vapour phase + y2(i)= K2(i)*x2;//mole fraction of propane in the vapour phase + y(i) = y1(i)+y2(i);//sum of the mole fraction in the vapour phase +end +plot(P,y); +xtitle("y vs pressure","P","y"); +P1 = interpln([y';P],1);// in Kgf/sq cm +mprintf('The bubble point pressure of the solution is %f Kgf/sq cm',P1); +//end \ No newline at end of file diff --git a/479/CH13/EX13.4/Example_13_4.sce b/479/CH13/EX13.4/Example_13_4.sce new file mode 100755 index 000000000..5c1116c47 --- /dev/null +++ b/479/CH13/EX13.4/Example_13_4.sce @@ -0,0 +1,37 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.4 +clear; +clc; + +//Given +T = [80.6 79.0 77.3 61.4];//Various temperature in deg cel +x1 = [0.0 15.0 29.0 100.0];//mole fraction of CHCl3 in liquid phase +y1 = [0.0 20.0 40.0 100.0];//mole fraction of CHCl3 in vapour phase +P1 = [1370 1310 1230 700];//Vapour pressure of CHCl3 in mm Hg +P = 760;//Total pressure in mm Hg + +//To Calculate the equilibrium data i.e y/x and compare with the experimental values +//From equation 13.27 (page no 245);K = y1/x1 = Pi/P +mprintf('Temperature Experimental Calculated'); + +for i = 1:4 + mprintf('\n %f',T(i)); + if x1(i) == 0 + mprintf(' Not defined'); + else + K_ex(i) = y1(i)/x1(i); +mprintf(' %f',K_ex(i)); + end +K_c(i) = P1(i)/P; +mprintf(' %f',K_c(i)); +end + +if K_ex(i) == K_c(i) + then mprintf('\n\n The liquid solution is perfect'); +else + mprintf('\n\n The liquid solution is imperfect'); +end +//end \ No newline at end of file diff --git a/479/CH13/EX13.5/Example_13_5.sce b/479/CH13/EX13.5/Example_13_5.sce new file mode 100755 index 000000000..72f3a8d68 --- /dev/null +++ b/479/CH13/EX13.5/Example_13_5.sce @@ -0,0 +1,11 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.5 +clear; +clc; + +//Given +//The given example is a theoretical problem and does not contain any numerical computation +//end \ No newline at end of file diff --git a/479/CH13/EX13.6/Example_13_6.sce b/479/CH13/EX13.6/Example_13_6.sce new file mode 100755 index 000000000..990304a97 --- /dev/null +++ b/479/CH13/EX13.6/Example_13_6.sce @@ -0,0 +1,24 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.6 +clear; +clc; + +//Given +x1 = 0.1;//Mole fraction of dichloromethane (CCl2H2) +x2 = 0.9;//Mole fraction of methyl acetate (C3H6O2) +M1 = 85;//Molecular weight of CCl2H2 +M2 = 74;//Molecular weight of C3H602 +D1 = 1.3163;//Density of CCl2H2 in gm/cc +D2 = 0.9279;//Density of C3H6O2 in gm/cc + +//To Calculate the volume of 10% dichloromethane solution +V1 = M1/D1;//Specific volume of pure CCL2H2 in cc/gmole +V2 = M2/D2;//Specific volume of C3H6O2 in cc/gmole +//From equation 13.62(page no 256)& 13.78 (page no 257) +V_e = x1*x2*(1.2672-0.771*x1);//excess volume in cc/gmole +V = V1*x1+V2*x2+V_e; +mprintf('The volume of 10 percent dichloromethane is %f cc/gmole',V); +//end \ No newline at end of file diff --git a/479/CH13/EX13.7/Example_13_7.sce b/479/CH13/EX13.7/Example_13_7.sce new file mode 100755 index 000000000..695af3a9d --- /dev/null +++ b/479/CH13/EX13.7/Example_13_7.sce @@ -0,0 +1,52 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.7 +clear; +clc; + +//Given +x_T = 0.957;//mole fraction of Toluene +x_D = 0.043;//mole fraction of 1,2-dichloroethane +t = [90; 100; 110];//temperature in deg cel +R = 1.98;//gas constant in Kcal/Kgmole K + +//To Calculate the vapour pressure of the solution, bubble point at 686 mm Hg and the vapour composition at equilibrium, +//compare the experimental value of 91.2% toluene in vapour with the calculated value & calculate the free energy of mixing +//(1)Calculation of vapour pressure +mprintf('(1)Temp(deg cel) P_T(mmHg) P_D(mmHg) P_s(mmHg)'); +for i = 1:3 + P_T(i) = 10^(6.95464-(1344.8/(219.482+t(i))));//Given as equation(a)(page no 260) + P_D(i) = 10^(7.03993-(1274.079/(223+t(i))));//Given as equation(b)(page no 260) + P_s(i) = x_T*P_T(i)+x_D*P_D(i);//pressure of the solution in mm Hg + mprintf('\n %f',t(i)); + mprintf(' %f',P_T(i)); + mprintf(' %f',P_D(i)); + mprintf(' %f',P_s(i)); +end + +//(2)Calculation of bubble point and comparison of values +clf; +plot(t,P_s); +xtitle("t vs P_s","t","P_s"); +T = interpln([P_s';t'],686); +P = 686;//pressure of solution in mm Hg +y_T_e = 0.912;//experimental value of mole fraction of toluene +//From the graph we found that the temperature at P = 686 mm Hg is +//t = 105.3;//in deg cel +mprintf('\n\n(2)The bubble point is %f deg cel',T); +//From equation (a)(page no 260) +P_T = 10^(6.95464-(1344.8/(219.482+T)));//vapour pressure of Toluene in mmHg +//From equation 13.27 (page no 245) +y_T_c = (x_T*P_T)/P; +y_D_c = 1-y_T_c; +mprintf('\n The vapour composition of toluene is %f',y_T_c); +mprintf('\n The vapour composition of 1,2-dichloroethane is %f',y_D_c); +e = ((y_T_e-y_T_c)/y_T_e)*100; +mprintf('\n The percentage error is %f percent',e); + +//(3)Calculation of free energy +del_F = R*(T+273)*((x_T*log(x_T))+(x_D*log(x_D))); +mprintf('\n\n(3)The free energy of mixing is %f Kcal/Kgmole',del_F); +//end \ No newline at end of file diff --git a/479/CH13/EX13.8/Example_13_8.sce b/479/CH13/EX13.8/Example_13_8.sce new file mode 100755 index 000000000..2699ffb34 --- /dev/null +++ b/479/CH13/EX13.8/Example_13_8.sce @@ -0,0 +1,26 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.8 +clear; +clc; + +//Given +//Consider the diagram shown in page no 263 +w1 = 100;//weight of LiBr entered as feed in the evaporator per hour in Kg +x1 = 0.45;//weight fraction of LiBr entered as feed +x2 = 0;//weight fraction of steam in the LiBr soln +x3 = 0.65;//weight fraction of LiBr formed as product +H1 = -39;//Enthalpy of 45% solution at 25 deg cel in Kcal/Kg +H3 = -4.15;//Enthalpy of 65% solution at 114.4 deg cel in Kcal/Kg +H2 = 649;//Enthalpy of superheated steam at 100 mmHg and 114.4 deg cel in Kcal/Kg + +//To Calculate the heating load required for the process +//According to material balance +w3 = (w1*x1)/x3;//weight of LiBr solution formed after evaporation per hour in Kg +w2 = w1-w3;// weight of steam formed in Kg/hr +//According to energy balance +Q = (w2*H2)+(w3*H3)-(w1*H1); +mprintf('The heat that has to be supplied for this concentration process is %f Kcal/hr',Q); +//end \ No newline at end of file diff --git a/479/CH13/EX13.9/Example_13_9.sce b/479/CH13/EX13.9/Example_13_9.sce new file mode 100755 index 000000000..b260581f6 --- /dev/null +++ b/479/CH13/EX13.9/Example_13_9.sce @@ -0,0 +1,11 @@ +//Chemical Engineering Thermodynamics +//Chapter 13 +//Thermodynamics in Phase Equilibria + +//Example 13.9 +clear; +clc; + +//Given +// In the given example, all the values were determined from the graph given as figure 13.9 and it does not involve any numerical computation +//end \ No newline at end of file -- cgit