initial commit / add all books

12 files changed, 176 insertions, 0 deletions

diff --git a/2006/CH14/EX14.1/ex14_1.sce b/2006/CH14/EX14.1/ex14_1.sce
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index 000000000..7b8d0554e
--- /dev/null
+++ b/2006/CH14/EX14.1/ex14_1.sce
@@ -0,0 +1,6 @@
+clc;

+// From the Table 14.1 

+del_hfHCL=92307; // Enthalpy of Heat in kJ/kmol

+del_hfH2O=-241818; // Enthalpy of Heat kJ/kmol

+del_Ho=4*del_hfHCL-2*del_hfH2O; // The standard heat of reaction from enthalpy equation

+disp ("kJ   (answer mentioned in the textbook is wrong)",del_Ho,"The standard heat of reaction for the process = ");

diff --git a/2006/CH14/EX14.10/ex14_10.sce b/2006/CH14/EX14.10/ex14_10.sce
new file mode 100755
index 000000000..796916a22
--- /dev/null
+++ b/2006/CH14/EX14.10/ex14_10.sce
@@ -0,0 +1,29 @@
+clc;

+// (a).The product CO2 is also at 298K

+Pco=2/3; // Paratial pressure of CO in atm 

+Po2=1/3; // Paratial pressure of O2 in atm

+Pco2=1; // Paratial pressure of CO2 in atm

+T0=298; // Temperature of surroundings in kelvin

+R_1=8.3143; // Universal gas constant of air in kJ/kmol K

+// From table 14.1 at 298 K and 1 atm

+s_co2=213.795-R_1*log (Pco2); // entropies in kJ/kmol K

+s_co=197.653-R_1*log (Pco); // entropies in kJ/kmol K

+s_o2=205.03-R_1*log (Po2); // entropies in kJ/kmol K

+del_Scv=s_co2-s_co-1/2*s_o2; // Entropy change of comtrol volume 

+// From table 14.1

+del_hfco2=-393509; del_hfco=-110525; // Enthalpy of Heat in kJ/kmol

+Q= del_hfco2- del_hfco; // Heat transfer (to surroundings)

+del_Ssurr=abs(Q)/T0; // Entropy change of surroundings

+del_Sgen=del_Scv+del_Ssurr; //Entropy change of universe

+disp ("kJ/K",del_Sgen,"Entropy change of universe = ","kJ/K",del_Ssurr,"Entropy change of surroundings = ","kJ/K",del_Scv,"Entropy change of comtrol volume  = ","(a).The product CO2 is also at 298K");

+// (b).The reaction is adiabatic

+// Let the adiabatic flame temperature be T. Then since

+Q=0;

+C_p=44*0.8414;

+// From table A.16

+T=5057.5; //adiabatic flame temperature in kelvin

+s_CO2=213.795+C_p*log (T/T0); // entropies in kJ/kmol K

+del_Scv=s_CO2-s_co-1/2*s_o2; // Entropy change of comtrol volume 

+del_Ssurr=abs(Q)/T0; // Entropy change of surroundings

+del_Sgen=del_Scv+del_Ssurr; //Entropy change of universe

+disp ("kJ/K",del_Sgen,"Entropy change of universe = ","kJ/K",del_Ssurr,"Entropy change of surroundings = ","kJ/K",del_Scv,"Entropy change of comtrol volume  = ","(b).The reaction is adiabatic");

diff --git a/2006/CH14/EX14.11/ex14_11.sce b/2006/CH14/EX14.11/ex14_11.sce
new file mode 100755
index 000000000..00c9585b3
--- /dev/null
+++ b/2006/CH14/EX14.11/ex14_11.sce
@@ -0,0 +1,11 @@
+clc;

+// The Combustion of H2 with Q2 from H2O

+//H2(g)+1/2 O2 (g)→H2O(l)+285830 kJ/kmol H2

+T0=298; // Temperature of surroundings in kelvin

+// From table 14.1 at 298 K

+del_hfH2O=-285830; // Enthalpy of Heat in kJ/kmol

+s_298H2O=69.94; s_298H2=130.684; s_298O2=205.142; // entropies in kJ/kmol K

+GP_GR=del_hfH2O-T0*(s_298H2O-s_298H2-1/2*s_298O2); // Formation of Gibbs function

+GR=0;

+GP=GP_GR-GR; // Standard Gibbs function of formation of liquid H2O

+disp ("kJ/kmol",GP,"Standard Gibbs function of formation of liquid H2O = ");

diff --git a/2006/CH14/EX14.12/ex14_12.sce b/2006/CH14/EX14.12/ex14_12.sce
new file mode 100755
index 000000000..bec785529
--- /dev/null
+++ b/2006/CH14/EX14.12/ex14_12.sce
@@ -0,0 +1,22 @@
+clc;

+// the combustion equation

+// n1C3H8+n2O2+n3 N2 → n4 CO2+ n5 H2O+n6 O2+n7 N2

+T0=298; // Temperature of surroundings in kelvin

+// (a).Product species at 25 oC and 1 atm

+d_gfC3H8=-24290; d_gfCO2=-394359; d_gfH2O=-228570; // in kJ/kmol

+GR=d_gfC3H8;

+GP=3*d_gfCO2+4*d_gfH2O;

+Wmax=GR-GP; // Maximum possible work output

+M=44;//Molecular weight

+Wmax=Wmax/M;

+disp ("kJ/kg fuel   (answer mentioned in the textbook is wrong)",Wmax,"Maximum possible work output = ","(a).");

+// (b).The actual partial pressures of products

+n1=1; n2=20; n3=75.2;

+n4=3; n5=4; n6=15; n7=75.2; // refer equation

+SR=19233; SP=19147; // in kJ/K from table

+HR=-104680; // in kJ/kmol fuel

+d_h0fCO2=-393509; d_h0fH2O=-241818; // in kJ/kmol

+HP=3*d_h0fCO2+4*d_h0fH2O;

+Wmax=HR-HP-T0*(SR-SP); // Maximum possible work output

+Wmax=Wmax/M;

+disp ("kJ/kg   (round off error)",Wmax,"Maximum possible work output = ","(b).");

diff --git a/2006/CH14/EX14.2/ex14_2.sce b/2006/CH14/EX14.2/ex14_2.sce
new file mode 100755
index 000000000..7dbf1df8a
--- /dev/null
+++ b/2006/CH14/EX14.2/ex14_2.sce
@@ -0,0 +1,6 @@
+clc;

+del_Ho=5640000; // Heat released during the process

+// From the Table 14.1 

+del_hfO2=-393509; del_hfH2O=-285830; // Enthalpy of Heat in kJ/kmol

+del_hfsucrose=12*del_hfO2+11*del_hfH2O+del_Ho; // The enthalpy formation of sucrose

+disp ("kJ/kmol   (answer mentioned in the textbook is wrong)",del_hfsucrose,"The enthalpy formation of sucrose = ");

diff --git a/2006/CH14/EX14.3/ex14_3.sce b/2006/CH14/EX14.3/ex14_3.sce
new file mode 100755
index 000000000..162819364
--- /dev/null
+++ b/2006/CH14/EX14.3/ex14_3.sce
@@ -0,0 +1,16 @@
+clc;

+// (a).Balancing of chemical equation

+// The unbalanced equation for the process is C8H18 + O2 + N2 → CO2 + H2O + N2

+x=8; // Carbon balance

+y=9; // Hydrogen balance

+z=12.5; // Oxygen balance in reverse order

+n=z*3.76; // Nitrogen Balance

+disp ("(a).Balancing of chemical equation");

+printf ("\n C8H18 + %0.1f O2 + %d N2 → %d CO2 + %d H2O + %d N2 \n ",z,n,x,y,n);

+// (b).The theoretical air-fuel ratio

+a=1; // Mole of C8H18

+AF1=(z+n)/a; //The theoretical air-fuel ratio on mole basis

+ma=28.84; // Molecular mass of air 

+mc=114; // Molecular mass of C8H18

+AF2=(AF1*ma)/(a*mc); // The theoretical air-fuel ratio on mass basis

+disp ("kg air / kmol C8H18",AF2,"The theoretical air-fuel ratio on mass basis = ","kmol air / kmol C8H18",AF1,"The theoretical air-fuel ratio on mole basis = ","(b).The theoretical air-fuel ratio");

diff --git a/2006/CH14/EX14.4/ex14_4.sce b/2006/CH14/EX14.4/ex14_4.sce
new file mode 100755
index 000000000..59fbbf9dc
--- /dev/null
+++ b/2006/CH14/EX14.4/ex14_4.sce
@@ -0,0 +1,8 @@
+clc;

+// The combustion equation for C4H10 with 80% theoretical air is C4H10 +5.2(O2 + 3.76 N2) → a(1)CO + a(2)CO2 + 5H2O + 19.55N2

+// The following matrix shows the balance of C and O

+A=[1 1 ; 1 2];

+B=[4 ;5.4];

+a=A\B;

+disp ("The equation for the combustion of butane with 80% theoretical air is ")

+printf ("\n C4H10 +5.2(O2 + 3.76 N2) → %0.1f CO + %0.1f CO2 + 5H2O + 19.55N2",a(1),a(2));

diff --git a/2006/CH14/EX14.5/ex14_5.sce b/2006/CH14/EX14.5/ex14_5.sce
new file mode 100755
index 000000000..aa64da71f
--- /dev/null
+++ b/2006/CH14/EX14.5/ex14_5.sce
@@ -0,0 +1,16 @@
+clc;

+p=101.325; // Atmospheric pressure in kPa

+// The complete combustion equation for actane

+ // yC8H18+ x (O2+3.76N2)  → n1 CO2+n2 H2O+n3 O2+n3 N2

+x=12.5*1.5; y=1;

+n1=8; n2=9; n3=6.28; n4=70.5;

+n=n1+n2+n3+n4; // Total number of moles of the products

+AFm=(x+x*3.76)/y ;// Air fuel ratio

+m=28.84;

+M=116; // Molecular weight of octane

+AF=AFm*m/M;

+yco2=n1/n; yH2O=n2/n; yO2=n3/n; yN2=n4/n;

+pH2O=p*yH2O; // Partial pressure of water vapour in the products

+Tsat=45.21; // In oC

+disp ("kg air/kg octane",AF,"Air fuel ratio = ");

+disp ("If the products are cooled below 25 oC then,  the water vapour will condense. Because the cooled temperature is less than dew point temperature of water vapour i.e., T < Tsat.");

diff --git a/2006/CH14/EX14.6/ex14_6.sce b/2006/CH14/EX14.6/ex14_6.sce
new file mode 100755
index 000000000..ec8d04571
--- /dev/null
+++ b/2006/CH14/EX14.6/ex14_6.sce
@@ -0,0 +1,23 @@
+clc;

+// The complete chemical equation is                                            //[0.14H2+0.03CH4+0.27CO+0.045CO2+0.01O2+0.505N2]+0.255(O2+3.75N2) →0.2H2O+0.345CO2+1.44N2

+a=0.14; // Composition of H2 in air

+b=0.03; // Composition of CH4 in air

+c=0.27; // Composition of CO in air

+d=0.045; // Composition of CO2 in air

+e=0.01; // Composition of O2 in air

+f=0.505; // Composition of N2 in air

+g=(0.265-0.01); // O2 requirement from atmospheric air with 1% O2 already in fuel

+h=3.76; // By nitrogen balance 

+i=1; // mole of the air

+AFvol=(g+(g*h))/i; // Air fuel ratio (theroretical)

+AFv=1.1*AFvol; // Air fuel ratio on mol (volume) basis

+disp ("kmol actual air/kmol fuel",AFv,"Air fuel ratio on mol (volume) basis =")

+M1=2; // Molecular mass of H2

+M2=16; // Molecular mass of CH4

+M3=28; // Molecular mass of CO

+M4=44; // Molecular mass of CO2

+M5=32; // Molecular mass of O2

+M=a*M1+b*M2+c*M3+d*M4+e*M5+f*M3; // Molecular mass of Fuel

+Ma=28.84; // Molecular mass of air

+AFm=AFv*Ma/(i*M); // Air fuel ratio on mass basis

+disp ("kg air / kg fuel",AFm,"Air fuel ratio on mass basis = ");

diff --git a/2006/CH14/EX14.7/ex14_7.sce b/2006/CH14/EX14.7/ex14_7.sce
new file mode 100755
index 000000000..85812cd57
--- /dev/null
+++ b/2006/CH14/EX14.7/ex14_7.sce
@@ -0,0 +1,16 @@
+clc;

+//From table 14.2 at 25 oC and 1 atm for C8H8

+del_Ho=-2039.7; // LHV in MJ/kmol

+// Combustion equation is C3H8+ 5O2 +18.8N2 → 3CO2 +4H2O +18.8N2

+// From table 14.3

+h333_C3H8=2751; // h333_h298 of C3H8 in kJ/kmol

+h333_O2=147; // h333_h298 of O2 in kJ/kmol

+h333_N2=145; // h333_h298 of N2 in kJ/kmol

+h1333_CO2=52075; // h1333_h298 of CO2 in kJ/kmol

+h1333_H2O=32644; // h1333_h298 of H2O in kJ/kmol

+h1333_N2=32644; // h1333_h298 of N2 in kJ/kmol

+M=44; // molecular mass of C3H8

+Ha_H1=h333_C3H8+5*h333_C3H8+18.8*h333_N2; // The enthalpy differences

+Hb_H2=3*h1333_CO2+4*h1333_H2O+18.8*h1333_N2; // The enthalpy differences

+Q=(del_Ho+Hb_H2/1000-Ha_H1/1000)/M; // Heat transfer from combustion chamber

+disp ("MJ/kg C3H8",abs (Q),"Heat transfer from combustion chamber =");

diff --git a/2006/CH14/EX14.8/ex14_8.sce b/2006/CH14/EX14.8/ex14_8.sce
new file mode 100755
index 000000000..33622f7c9
--- /dev/null
+++ b/2006/CH14/EX14.8/ex14_8.sce
@@ -0,0 +1,7 @@
+clc;

+Ha_H1=6220; // From example 14.7 in kJ/kmol

+del_Ho=-2039.7; // From example 14.7 LHV in MJ/kmol

+Hb_H2=-del_Ho+Ha_H1; // For adiabatic combustion of C3H8

+// Hb_H2=3*h1333_CO2+4*h1333_H2O+18.8*h1333_N2 By iteration process and making use of the values from Table A.3, A.13, A.15 we can get the adiabatic flame temperature is

+Tad=2300;// The adiabatic flame temperature in kelvin

+disp ("K",Tad,"The adiabatic flame temperature");

diff --git a/2006/CH14/EX14.9/ex14_9.sce b/2006/CH14/EX14.9/ex14_9.sce
new file mode 100755
index 000000000..5da736239
--- /dev/null
+++ b/2006/CH14/EX14.9/ex14_9.sce
@@ -0,0 +1,16 @@
+clc;

+// (a).Entropy change per kmol of C

+// From table 14.1 at 298 K and 1 atm

+s_c=5.686; // Absolute entropies of C in kJ/kmol K

+s_o2=205.142; // Absolute entropies of o2 in kJ/kmol K

+s_co2=213.795; // Absolute entropies of CO2 in kJ/kmol K

+del_s=s_co2-(s_c+s_o2); // The entropy change 

+disp ("kJ/K/kmol C",del_s,"(a).The entropy change = ");

+// (b).Entropy change of universe

+Tsurr=298; // Temperature of surroundings in kelvin

+// From table 14.1 

+del_Ho=-393509; // del_hfco2 in kJ/kmol CO2

+Q=abs (del_Ho);

+del_Ssurr=Q/Tsurr; // Entropy change of surroundings

+del_Suniv=del_s+del_Ssurr; //Entropy change of universe

+disp ("kJ/K",del_Suniv,"(b).Entropy change of universe = ");