2 files changed, 98 insertions, 98 deletions
diff --git a/479/CH14/EX14.12/Example_14_12.sce b/479/CH14/EX14.12/Example_14_12.sce
index da72bbb33..def054a07 100755
--- a/479/CH14/EX14.12/Example_14_12.sce
+++ b/479/CH14/EX14.12/Example_14_12.sce
@@ -1,37 +1,37 @@
-//Chemical Engineering Thermodynamics
-//Chapter 14
-//Thermodynamics of Chemical Reactions
-
-//Example 14.12
-clear;
-clc;
-
-//Given
-//C + 2H2 - CH4
-//Basis: 1 Kgmole of C fed
-T = 1000;//Temperature in K
-P1 = 2;//Pressure in atm
-del_F = 4580;//Standard free energy in Kcal/Kgmole
-
-
-//To Calculate the maximum CH4 concentration under the condition of 2 atm and the  quantity of methane obtained if pressure is 1 atm
-Ka = %e^(-del_F/(R*T));//Equilibrium constant
-//In relation (d) (page no 339) p_H2 = p (say)
-p = poly(0,'p');
-q = Ka*(p^2)+p-P1;
-r = roots(q);
-p_H2 = r(2);//partial pressure of H2
-p_CH4 = P1-p_H2;//partial pressure of CH4
-X_H2 = p_H2*100/P1;//mole percent of H2
-X_CH4 = p_CH4*100/P1;//mole percent of CH4
-mprintf('Under the conditions of 2 atm and 1000 K,the maximum CH4 concentration is %f percent and further increase is not pssible',X_CH4);
-//Now.pressure has become
-P2 = 1;//in atm
-q = Ka*(p^2)+p-P2;
-r = roots(q);
-p_H2 = r(2);//partial pressure of H2
-p_CH4 = P2-p_H2;//partial pressure of CH4
-X_H2 = p_H2*100/P2;//mole percent of H2
-X_CH4 = p_CH4*100/P2;//mole percent of CH4
-mprintf('\n\n Under the conditions of 1 atm and 1000 K,Methane = %f percent and Hydrogen = %f percent',X_CH4,X_H2);
+//Chemical Engineering Thermodynamics
+//Chapter 14
+//Thermodynamics of Chemical Reactions
+
+//Example 14.12
+clear;
+clc;
+
+//Given
+//C + 2H2 - CH4
+//Basis: 1 Kgmole of C fed
+T = 1000;//Temperature in K
+P1 = 2;//Pressure in atm
+del_F = 4580;//Standard free energy in Kcal/Kgmole
+R = 1.98;
+
+//To Calculate the maximum CH4 concentration under the condition of 2 atm and the  quantity of methane obtained if pressure is 1 atm
+Ka = %e^(-del_F/(R*T));//Equilibrium constant
+//In relation (d) (page no 339) p_H2 = p (say)
+p = poly(0,'p');
+q = Ka*(p^2)+p-P1;
+r = roots(q);
+p_H2 = r(2);//partial pressure of H2
+p_CH4 = P1-p_H2;//partial pressure of CH4
+X_H2 = p_H2*100/P1;//mole percent of H2
+X_CH4 = p_CH4*100/P1;//mole percent of CH4
+mprintf('Under the conditions of 2 atm and 1000 K,the maximum CH4 concentration is %f percent and further increase is not pssible',X_CH4);
+//Now.pressure has become
+P2 = 1;//in atm
+q = Ka*(p^2)+p-P2;
+r = roots(q);
+p_H2 = r(2);//partial pressure of H2
+p_CH4 = P2-p_H2;//partial pressure of CH4
+X_H2 = p_H2*100/P2;//mole percent of H2
+X_CH4 = p_CH4*100/P2;//mole percent of CH4
+mprintf('\n\n Under the conditions of 1 atm and 1000 K,Methane = %f percent and Hydrogen = %f percent',X_CH4,X_H2);
 //end
 \ No newline at end of file
diff --git a/479/CH14/EX14.6/Example_14_6.sce b/479/CH14/EX14.6/Example_14_6.sce
index e81c94b47..f7ac46d6d 100755
--- a/479/CH14/EX14.6/Example_14_6.sce
+++ b/479/CH14/EX14.6/Example_14_6.sce
@@ -1,63 +1,63 @@
-//Chemical Engineering Thermodynamics
-//Chapter 14
-//Thermodynamics of Chemical Reactions
-
-//Example 14.6
-clear;
-clc;
-
-//Given
-//SO2 + (1/2)O2 - SO3
-//Basis: 1 Kgmole of SO2
-n_SO2 = 1;// SO2 fed in Kgmole
-//From table 14.1 (page no 301)
-//alpha values for the following components are given as
-a_SO2 = 7.116;
-a_O2 = 6.148;
-a_SO3 = 6.077;
-//beta values for the following components are given as
-b_SO2 = 9.512*10^-3;
-b_O2 = 3.102*10^-3;
-b_SO3 = 25.537*10^-3;
-//Standard enthalpy of the following components at 25 deg cel in Kcal/Kgmole are given as
-H_SO2 -70960;
-H_O2 = 0;
-H_SO3 = -94450;
-//Standard free energy of the following components at 25 deg cel in Kcal/Kgmole K are given as
-F_SO2 = -71680;
-F_O2 = 0;
-F_SO3 = -88590;
-n_O2 = n_SO2;//O2 fed in Kgmole; since 50 mole percent mixture of SO2 & O2 is fed
-n_SO3 = n_SO2;//SO3 formed in Kgmole
-n_O2_e = n_O2-(n_O2/2);//Kgmoles of O2 in exit gas
-n_O2_r = n_O2/2;//Kgmoles of O2 reacted
-R = 1.98;//gas constant in Kcal/Kgmole K
-
-//To show  the variation of the standard heats of reaction with temperature and the equilibrium constant with temperature graphically in the  given temperature range
-//(i)Variation of the standard heats of reaction with temperature
-del_H = (n_SO3*H_SO3)-(n_O2_r*H_O2)-(n_SO2*H_SO2);// in Kcal/Kgmole
-del_F = (n_SO3*F_SO3)-(n_O2_r*F_O2)-(n_SO2*F_SO2);// in Kcal/Kgmole
-//From equation 14.10 (page no 301)
-del_a = (n_SO3*a_SO3)-(n_O2_r*a_O2)-(n_SO2*a_SO2);
-del_b = (n_SO3*b_SO3)-(n_O2_r*b_O2)-(n_SO2*b_SO2);
-//In equation 14.11 (page no 302), substituting del_H at
-T = 298;//in deg cel
-I = del_H - del_a*T - (del_b*(T^2)/2);// integrating constant
-mprintf('(i)The standard heat of reaction at any tempperature can be calculated by the relation:');
-mprintf('\n    del_Ht = %fT + %fT^2 %f',del_a,del_b/2,I);
-
-//(ii)Variation of the equilibrium constant with temperature
-//K1 = lnKa (say)
-K1 = -del_F/(R*T);
-//From equation 14.42 (page no 316); M1 = M/R (say)
-M1 = K1-(del_a/R)*log(T)-(del_b/(2*R))*T+(I/(T*R));
-//Let us assume the temperature in the range 800K to 1500K as
-Ta = [700 800 825 850 900 1000 1100 1300 1500];
-for i = 1:9
-    Ka(i) = %e^((del_a/R)*log(Ta(i))+(del_b*Ta(i)/(2*R))-(I/(Ta(i)*R))+M1);
-end
-clf;
-plot(Ta,Ka);
-xtitle(" ","Temperature in K","equilibrium constant K");
-mprintf('\n\n(ii)From the graph it can be seen that as temperature increases Ka decreases exponentially,so the reaction is exothermic.');
+//Chemical Engineering Thermodynamics
+//Chapter 14
+//Thermodynamics of Chemical Reactions
+
+//Example 14.6
+clear;
+clc;
+
+//Given
+//SO2 + (1/2)O2 - SO3
+//Basis: 1 Kgmole of SO2
+n_SO2 = 1;// SO2 fed in Kgmole
+//From table 14.1 (page no 301)
+//alpha values for the following components are given as
+a_SO2 = 7.116;
+a_O2 = 6.148;
+a_SO3 = 6.077;
+//beta values for the following components are given as
+b_SO2 = 9.512*10^-3;
+b_O2 = 3.102*10^-3;
+b_SO3 = 25.537*10^-3;
+//Standard enthalpy of the following components at 25 deg cel in Kcal/Kgmole are given as
+H_SO2 =-70960;
+H_O2 = 0;
+H_SO3 = -94450;
+//Standard free energy of the following components at 25 deg cel in Kcal/Kgmole K are given as
+F_SO2 = -71680;
+F_O2 = 0;
+F_SO3 = -88590;
+n_O2 = n_SO2;//O2 fed in Kgmole; since 50 mole percent mixture of SO2 &amp; O2 is fed
+n_SO3 = n_SO2;//SO3 formed in Kgmole
+n_O2_e = n_O2-(n_O2/2);//Kgmoles of O2 in exit gas
+n_O2_r = n_O2/2;//Kgmoles of O2 reacted
+R = 1.98;//gas constant in Kcal/Kgmole K
+
+//To show  the variation of the standard heats of reaction with temperature and the equilibrium constant with temperature graphically in the  given temperature range
+//(i)Variation of the standard heats of reaction with temperature
+del_H = (n_SO3*H_SO3)-(n_O2_r*H_O2)-(n_SO2*H_SO2);// in Kcal/Kgmole
+del_F = (n_SO3*F_SO3)-(n_O2_r*F_O2)-(n_SO2*F_SO2);// in Kcal/Kgmole
+//From equation 14.10 (page no 301)
+del_a = (n_SO3*a_SO3)-(n_O2_r*a_O2)-(n_SO2*a_SO2);
+del_b = (n_SO3*b_SO3)-(n_O2_r*b_O2)-(n_SO2*b_SO2);
+//In equation 14.11 (page no 302), substituting del_H at
+T = 298;//in deg cel
+I = del_H - del_a*T - (del_b*(T^2)/2);// integrating constant
+mprintf('(i)The standard heat of reaction at any tempperature can be calculated by the relation:');
+mprintf('\n    del_Ht = %fT + %fT^2 %f',del_a,del_b/2,I);
+
+//(ii)Variation of the equilibrium constant with temperature
+//K1 = lnKa (say)
+K1 = -del_F/(R*T);
+//From equation 14.42 (page no 316); M1 = M/R (say)
+M1 = K1-(del_a/R)*log(T)-(del_b/(2*R))*T+(I/(T*R));
+//Let us assume the temperature in the range 800K to 1500K as
+Ta = [700 800 825 850 900 1000 1100 1300 1500];
+for i = 1:9
+    Ka(i) = %e^((del_a/R)*log(Ta(i))+(del_b*Ta(i)/(2*R))-(I/(Ta(i)*R))+M1);
+end
+clf;
+plot(Ta,Ka);
+xtitle(" ","Temperature in K","equilibrium constant K");
+mprintf('\n\n(ii)From the graph it can be seen that as temperature increases Ka decreases exponentially,so the reaction is exothermic.');
 //end
 \ No newline at end of file