12 files changed, 219 insertions, 0 deletions
diff --git a/926/CH8/EX8.2/Chapter8_Example2.sce b/926/CH8/EX8.2/Chapter8_Example2.sce
new file mode 100644
index 000000000..d62429dc2
--- /dev/null
+++ b/926/CH8/EX8.2/Chapter8_Example2.sce
@@ -0,0 +1,38 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 2, Page 275
+//Title: Calculation of molal heat of vapourization
+//=============================================================================
+clear
+clc
+
+//INPUT
+P = [1 8]; //Given pressure in atm
+Tb = [56.5 133.1]; //Boiling point of acetone at 1 atm and 8 atm pressure in degree C
+TC = 508.7; //Critical temperature of acetone in K
+PC = 46.6; //Critical pressure of acetone in atm
+Com_fac = [.966 .822]; //(ZG - ZL) value of acetone at 1 and 8 atm respectively from Table 26A, Page 275
+A = 3.0644; //Vapor pressure constant of acetone from Table 8, Page 95
+b = .180; //Vapor pressure constant of acetone from Table 8, Page 95
+R = 1.987; //gas constant in 
+
+//CALCULATION
+TB = Tb+273.15; //Boiling point of acetone at 1 atm and 8 atm pressure in K
+TR = TB/TC; //reduced temperature of acetone at 1 and 8 atm pressure respectively in degree C
+lamda = 2.303*Com_fac*R*TC*A;
+lamda1 = 2.303*Com_fac(1)*R*TC*(A+(40*TR(1)^2*(TR(1)-b)*exp(-20*(TR(1)-b)^2)));
+lamda2 = 2.303*Com_fac(2)*R*TC*(A+(40*TR(2)^2*(TR(2)-b)*exp(-20*(TR(2)-b)^2)));
+
+//OUTPUT
+// Console Output
+mprintf('\n Molal heat of vaporization of acetone at \n   1 atm pressure         8 atm pressure: \n   %4.0f cal/g-mole        %4.0f cal/g-mole   -------from equation (32), Page 275 \n   %4.0f cal/g-mole        %4.0f cal/g-mole   -------from equation (33), page 275',lamda1,lamda2,lamda(1),lamda(2));
+
+// File output
+fd= mopen('.\Chapter8_Example2_Output.txt','w');
+mfprintf(fd,'\n Molal heat of vaporization of acetone at \n   1 atm pressure         8 atm pressure: \n   %4.0f cal/g-mole        %4.0f cal/g-mole   -------from equation (32), Page 275 \n   %4.0f cal/g-mole        %4.0f cal/g-mole   -------from equation (33), Page 275',lamda1,lamda2,lamda(1),lamda(2));
+mclose(fd);
+
+//=================================END OF PROGRAM==============================
+
+//Remarks
+//Difference between the solution computed by scilab and that given in book is due to round off error. The solution computed by scilab matches when the same is computed manually.
diff --git a/926/CH8/EX8.2/Chapter8_Example2_Output.txt b/926/CH8/EX8.2/Chapter8_Example2_Output.txt
new file mode 100644
index 000000000..9f82819c2
--- /dev/null
+++ b/926/CH8/EX8.2/Chapter8_Example2_Output.txt
@@ -0,0 +1,5 @@
+
+ Molal heat of vaporization of acetone at 
+   1 atm pressure         8 atm pressure: 
+   7112 cal/g-mole        5878 cal/g-mole   -------from equation (32), Page 275 
+   6891 cal/g-mole        5864 cal/g-mole   -------from equation (33), Page 275
+\ No newline at end of file
diff --git a/926/CH8/EX8.3/Chapter8_Example3.sce b/926/CH8/EX8.3/Chapter8_Example3.sce
new file mode 100644
index 000000000..888c33113
--- /dev/null
+++ b/926/CH8/EX8.3/Chapter8_Example3.sce
@@ -0,0 +1,28 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 3, Page 278
+//Title: Calculation of heat of vaporization
+//=============================================================================
+clear
+clc
+
+//INPUT
+T = 200; //Given temperature in degree F
+TC = 232.5; //Critical temperature of Freon 12 in degree F
+SRTR  = .516; //Heat of vaporization factor of Freon 12 from Table 27, Page 278
+
+//CALCULATION
+TR = (T+460)/(TC+460); //Reduced temperature of freon 12 at 200 degree F
+Lamda_1 = 7707; //Molal heat of vaporization of water at TR=0.951 in BTU per lb-mole obtained from Table page 279
+Lamda_2 = Lamda_1*SRTR; //Heat of vaporization of freon 12 at 200 degree F
+
+//OUTPUT
+// Console Output
+mprintf('\n Heat of vaporization of freon 12 at 200 degree F = %4.0f BTU per lb-mole',Lamda_2);
+
+// File Output
+fd= mopen('.\Chapter8_Example3_Output.txt','w');        // PRN: File name and path changed NAR 
+mfprintf(fd,'\n Heat of vaporization of freon 12 at 200 degree F = %4.0f BTU per lb-mole',Lamda_2);
+mclose(fd);
+
+//=================================END OF PROGRAM==============================
diff --git a/926/CH8/EX8.3/Chapter8_Example3_Output.txt b/926/CH8/EX8.3/Chapter8_Example3_Output.txt
new file mode 100644
index 000000000..38070c3ae
--- /dev/null
+++ b/926/CH8/EX8.3/Chapter8_Example3_Output.txt
@@ -0,0 +1,2 @@
+
+ Heat of vaporization of freon 12 at 200 degree F = 3977 BTU per lb-mole
+\ No newline at end of file
diff --git a/926/CH8/EX8.4/Chapter8_Example4.sce b/926/CH8/EX8.4/Chapter8_Example4.sce
new file mode 100644
index 000000000..787479ca4
--- /dev/null
+++ b/926/CH8/EX8.4/Chapter8_Example4.sce
@@ -0,0 +1,33 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 4, Page 281
+//Title: Calculation of heat of vaporization
+//=============================================================================
+clear
+clc
+
+//INPUT
+Tb = 78; //Normal boiling point of ethyl alcohol in degree C   
+Tc = 243; //Critical temperature of ethyl alcohol in degree C   
+T = 180; //Given temperature of ethyl alcohol in degree C   
+Lamda_1 = 204; //latent heat of vaporisation of ethyl alcohol at normal boiling point in cal per gram
+
+//CALCULATION
+TB = 273.15+Tb; //Normal boiling point of ethyl alcohol in K   
+TC = 273.15+Tc; //Critical temperature of ethyl alcohol in K
+T1 = 273.15+T; //Given temperature of ethyl alcohol in K 
+
+Tr1 = TB/TC; //Reduced temperature with reference to boiling point
+Tr2 = T1/TC; //Reduced temperature with reference to temperature at which heat of vaporization is to be estimated
+Lamda_2 = Lamda_1*((1-Tr2)/(1-Tr1))^0.38; //Heat of vaporization at given temperature in cal per gram
+
+//OUTPUT
+// Console Output
+mprintf('\n Heat of vaporization at a temperature of %3.0f degree C = %3.0f cal per gram',Tb,Lamda_2);
+
+// File Output
+fd= mopen('.\Chapter8_Example4_Output.txt','w');
+mfprintf(fd,'\n Heat of vaporization at a temperature of %3.0f degree C = %3.0f cal per gram',Tb,Lamda_2);
+mclose(fd);
+
+//=============================END OF PROGRMAM=================================
diff --git a/926/CH8/EX8.4/Chapter8_Example4_Output.txt b/926/CH8/EX8.4/Chapter8_Example4_Output.txt
new file mode 100644
index 000000000..30bf68959
--- /dev/null
+++ b/926/CH8/EX8.4/Chapter8_Example4_Output.txt
@@ -0,0 +1,2 @@
+
+ Heat of vaporization at a temperature of 180 degree C = 141 cal per gram
+\ No newline at end of file
diff --git a/926/CH8/EX8.5/Chapter8_Example5.sce b/926/CH8/EX8.5/Chapter8_Example5.sce
new file mode 100644
index 000000000..7a105fc42
--- /dev/null
+++ b/926/CH8/EX8.5/Chapter8_Example5.sce
@@ -0,0 +1,35 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 5, Page 281
+//Title: Calculation of enthalpy of steam
+//=============================================================================
+clear
+clc
+
+//INPUT
+T = [350 32]; //Given and liquid state temperature of steam in degree F
+P = 50; //Given pressure in psi
+TS = 281; //Saturation temperature of steam at 50 psi in degree F obtained from Table 5 Page 83
+CP1 = 1.006; //Mean specific heat of water between 32-281 degree F in BTU per lb degree F
+CP2 = 9.2; //Mean heat capacity of water vapor between 32-281 degree F in BTU per lb-mole degree F
+lamda1 = 924; //Latent heat of vaporization of water at 281 degree F in BTU per lb
+MW = 18; //Molecular weight of water in lb/lb-mole
+
+//CALCULATION
+lamda2 = (TS-T(2))*CP1; //Enthalpy of liquid water at 281 degree F in BTU per lb
+lamda3 = (T(1)-TS)*CP2/MW; //Superheat of vapor in BTU per lb
+lamda = lamda1+lamda2+lamda3; //Total enyhalpy in BTU per lb
+
+//OUTPUT
+// Console Output
+mprintf('\n Total enthalpy of 1 lb steam = %5.1f BTU per lb',lamda);
+
+// File Output
+fd= mopen('.\Chapter8_Example5_Output.txt','w');
+mfprintf(fd,'\n Total enthalpy of 1 lb steam = %5.1f BTU per lb',lamda);
+mclose(fd);
+
+//=============================END OF PROGRMAM=================================
+
+// Remark
+// Difference between the solution computed by scilab and that given in book is due to round off error. For instance, enthalpy computed by (281-32)*1.006 should be 250.494 and not 2501. as printed in the textbook.
diff --git a/926/CH8/EX8.5/Chapter8_Example5_Output.txt b/926/CH8/EX8.5/Chapter8_Example5_Output.txt
new file mode 100644
index 000000000..5bc70dc7f
--- /dev/null
+++ b/926/CH8/EX8.5/Chapter8_Example5_Output.txt
@@ -0,0 +1,2 @@
+
+ Total enthalpy of 1 lb steam = 1209.8 BTU per lb
+\ No newline at end of file
diff --git a/926/CH8/EX8.6/Chapter8_Example6.sce b/926/CH8/EX8.6/Chapter8_Example6.sce
new file mode 100644
index 000000000..5e344102c
--- /dev/null
+++ b/926/CH8/EX8.6/Chapter8_Example6.sce
@@ -0,0 +1,35 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 6, Page 282
+//Title: Calculation of total enthalpy
+//=============================================================================
+clear
+clc
+
+//INPUT
+AW = 65.4; //Atomic weight of zinc
+T = [1000 0 419 907]; //Given temperature, solid state temperature, melting point and boiling point of zinc in degree C
+CP = [0.105 0.109]; //Mean specific heat of solid from 0-419 degree C and liquid from 419-907 degree C in cal per gram degree C obtained from Fig 63, Page 260
+lamda1 = 1660; //Heat of fusion in cal per g-atom obtained from Table 24, Page 272
+CP1 = 4.97; //Molal heat capacity of zinc vapor at constant preesure in cal per g-mole
+
+//CALCULATION
+T1 = T+273; //Given temperature, solid state temperature, melting point and boiling point of zinc in K
+lamda2 = T1(4)*(8.75+4.571*log10(T1(4))); //Heat of vaporization at normal boiling point in cal per g-mole
+Lamda1 = CP(1)*(T(3)-T(2)); //Heat absorbed by solid in cal per gram
+Lamda2 = lamda1/AW; //Heat of fusion in cal per gram
+Lamda3 = CP(2)*(T(4)-T(3)); //Heat absorbed by liquid in cal per gram
+Lamda4 = lamda2/AW; //Heat of vaporization in cal per gram
+Lamda5 = CP1*(T(1)-T(4))/AW; //Heat absorbed by vapor in cal per gram
+Lamda = Lamda1+Lamda2+Lamda3+Lamda4+Lamda5; //Total enthalpy in cal per gram
+
+//OUTPUT
+// Console Output
+mprintf('\n Total enthalpy of zinc vapor at 1000 degree C = %3.0f cal per gram',Lamda);
+
+// File Output
+fd= mopen('.\Chapter8_Example6_Output.txt','w');
+mfprintf(fd,'\n Total enthalpy of zinc vapor at 1000 degree C = %3.0f cal per gram',Lamda);
+mclose(fd);
+
+//=============================END OF PROGRMAM=================================
diff --git a/926/CH8/EX8.6/Chapter8_Example6_Output.txt b/926/CH8/EX8.6/Chapter8_Example6_Output.txt
new file mode 100644
index 000000000..395b32efe
--- /dev/null
+++ b/926/CH8/EX8.6/Chapter8_Example6_Output.txt
@@ -0,0 +1,2 @@
+
+ Total enthalpy of zinc vapor at 1000 degree C = 541 cal per gram
+\ No newline at end of file
diff --git a/926/CH8/EX8.7/Chapter8_Example7.sce b/926/CH8/EX8.7/Chapter8_Example7.sce
new file mode 100644
index 000000000..98f908a51
--- /dev/null
+++ b/926/CH8/EX8.7/Chapter8_Example7.sce
@@ -0,0 +1,35 @@
+//Hougen O.A., Watson K.M., Ragatz R.A., 2004. Chemical process principles Part-1: Material and Energy Balances(II Edition). CBS Publishers & Distributors, New Delhi, pp 504
+
+//Chapter-8, Illustration 7, Page 283
+//Title: Calculation of total enthalpy
+//=============================================================================
+clear
+clc
+
+//INPUT
+T = [100 32]; //Given temperature and standard temperature of dry air in degree F
+MW = [18 29]; //Molecular weight of water and air respectively
+
+//DATA FROM GRAPH
+H = 0.0215; //humidity in terms of lb of water per lb of dry air at given conditions obtained from Fig 20, Page 122
+DP = 79; //Dew point corresponding to above humidity in degree F obtained from Fig 20, Page 122
+CP = [8.02 6.95]; //Molal heat capacities of water vapor between 79-100 degree F and 32-100 degree F in BTU per lb-mole degree F obtained from Fig 62, Page 259
+lamda = 1046; //Heat of vaporization at 79 degree F in BTU per lb obtained from Fig 19, Page 120
+
+//CALCULATION
+Lamda1 = (T(1)-T(2))*CP(2)/MW(2); //Sensible enthalpy of air in BTU per lb
+Lamda2 = (DP-T(2))*H; //Sensible enthalpy of liquid water in BTU per lb
+Lamda3 = lamda*H; //Latent heat of water in BTU per lb
+Lamda4 = (T(1)-DP)*H*CP(1)/MW(1); //Superheat of water vapor in BTU per lb
+Lamda = Lamda1+Lamda2+Lamda3+Lamda4; //Total enthalpy in BTU per lb of dry air
+
+//OUTPUT
+// Console Output
+mprintf('\n Total enthalpy of dry air is %2.0f BTU per lb',Lamda);
+
+// File Output
+fd= mopen('.\Chapter8_Example7_Output.txt','w');
+mfprintf(fd,'\n Total enthalpy of dry air is %2.0f BTU per lb',Lamda);
+mclose(fd);
+
+//=============================END OF PROGRMAM=================================
diff --git a/926/CH8/EX8.7/Chapter8_Example7_Output.txt b/926/CH8/EX8.7/Chapter8_Example7_Output.txt
new file mode 100644
index 000000000..b8465afba
--- /dev/null
+++ b/926/CH8/EX8.7/Chapter8_Example7_Output.txt
@@ -0,0 +1,2 @@
+
+ Total enthalpy of dry air is 40 BTU per lb
+\ No newline at end of file