initial commit / add all books

22 files changed, 319 insertions, 0 deletions

diff --git a/3856/CH4/EX4.1/Ex4_1.sce b/3856/CH4/EX4.1/Ex4_1.sce
new file mode 100644
index 000000000..2f0628268
--- /dev/null
+++ b/3856/CH4/EX4.1/Ex4_1.sce
@@ -0,0 +1,37 @@
+//Calculate the value of work done if the expansion is carried out against a vacuum ,against a constant external pressure of 1.00 atm and reversibly

+

+//Example 4.1

+

+clc;

+

+clear;

+

+n=0.850;  //Number of mole of gas in mol

+

+R1=0.08206; //Gas constant in L atm K^-1 mol^-1

+

+T=300;  //Temperature in K

+

+P1=15.0;  //Initial pressure in atm

+

+P2=1.00;  //Final pressure in atm

+

+Pex=0;  //Pressure in vaccum

+

+V1=(n*R1*T)/P1; //Initial volume

+

+V2=(n*R1*T)/P2;  //Final volume

+

+w1=-Pex*(V2-V1)*101.3;  //Work done against vaccum in J

+

+printf("(a)Work done if the expansion is carried out against a vaccum = %.0f J",w1);

+

+w2=-P2*(V2-V1)*101.3;  //Work done against a constant external pressure in J

+

+printf("\n(b)Value of work done if the expansion is carried out against a constant external pressure = %.2f*10^3 J",w2*10^-3);

+

+R2=8.314;  //Gas constant in J K^-1 mol^-1

+

+w3=(-n*R2*T)*log((P1/P2));  //Work done for an isothermal,reversible process in J

+

+printf("\n(c)Work done if the expansion is carried out for an isothermal,reversible process = %.2f*10^3 J",w3*10^-3);

diff --git a/3856/CH4/EX4.1/Ex4_1.txt b/3856/CH4/EX4.1/Ex4_1.txt
new file mode 100644
index 000000000..0965cb49a
--- /dev/null
+++ b/3856/CH4/EX4.1/Ex4_1.txt
@@ -0,0 +1,3 @@
+ (a)Work done if the expansion is carried out against a vaccum = -0 J

+(b)Value of work done if the expansion is carried out against a constant external pressure = -1.98*10^3 J

+(c)Work done if the expansion is carried out for an isothermal,reversible process = -5.74*10^3 J
\ No newline at end of file
diff --git a/3856/CH4/EX4.10/Ex4_10.sce b/3856/CH4/EX4.10/Ex4_10.sce
new file mode 100644
index 000000000..c2a015385
--- /dev/null
+++ b/3856/CH4/EX4.10/Ex4_10.sce
@@ -0,0 +1,25 @@
+//Calculate the standard Enthalpy  for the reaction three Oxygen molecule givs two Ozone molecule

+

+//Example 4.10

+

+clc;

+

+clear;

+

+delrH298deg=285.4;  //standard enthalpy at 298 k in kJ mol^-1

+

+Cp1=29.4;  //molar heat capacity for O2 at constant pressur in J K^-1

+

+Cp2=38.2;  //molar heat capacity for O3 at constant pressur in J K^-1

+

+delCp=2*Cp2-3*Cp1;  //change in molar heat capacity for reaction in J K^-1

+

+T2=380;  //final temperature in K

+

+T1=298;  //initial temperature in K

+

+delT=T2-T1;  //change in temperature in K

+ 

+delrH380deg=((delCp*delT)/1000)+delrH298deg;  //standard Enthalpy for the reaction at 380 K in kJ mol^-1

+

+printf("Standard Enthalpy = %.1f kJ mol^-1",delrH380deg);

diff --git a/3856/CH4/EX4.10/Ex4_10.txt b/3856/CH4/EX4.10/Ex4_10.txt
new file mode 100644
index 000000000..6bd5f11b9
--- /dev/null
+++ b/3856/CH4/EX4.10/Ex4_10.txt
@@ -0,0 +1 @@
+ Standard Enthalpy = 284.4 kJ mol^-1
\ No newline at end of file
diff --git a/3856/CH4/EX4.11/Ex4_11.sce b/3856/CH4/EX4.11/Ex4_11.sce
new file mode 100644
index 000000000..4e7d394ba
--- /dev/null
+++ b/3856/CH4/EX4.11/Ex4_11.sce
@@ -0,0 +1,29 @@
+// Estimate the Enthaply of Combustion for Methane

+

+//Exaample 4.11

+

+clc;

+

+clear;

+

+H1=414; //Bond Enthalpy for a C-H bond in kJ mol^-1

+

+H2=498.8; //Bond Enthalpy for a O-O bond in kJ mol^-1 

+

+H3=799;  //Bond Enthalpy for a C=O bond kJ mol^-1

+

+H4=460;  //Bond Enthalpy for a O-H bond kJ mol^-1

+

+delHr=((4*H1)+(2*H2))-((2*H3)+(4*H4)); //Enthalpy of the reaction kJ mol^-1

+

+printf("Enthalpy Change of combustion of methane = %.1f kJ mol^-1",delHr);

+

+H5=-393.5;  //Enthalpy of formation of CO2 kJ mol^-1

+

+H6=-241.8;  //Enthalpy of formation of H2O kJ mol^-1

+

+H7=-74.85;  //Enthalpy of formation of CH4 kJ mol^-1

+

+delHf=(H5+(2*H6))-H7; //Enthalpy of formation kJ mol^-1

+

+printf("\nEnthalpy Change of combustion of methane from enthalpy of formation = %.1f kJ mol^-1",delHf);

diff --git a/3856/CH4/EX4.11/Ex4_11.txt b/3856/CH4/EX4.11/Ex4_11.txt
new file mode 100644
index 000000000..f779270cd
--- /dev/null
+++ b/3856/CH4/EX4.11/Ex4_11.txt
@@ -0,0 +1,2 @@
+ Enthalpy Change of combustion of methane = -784.4 kJ mol^-1

+Enthalpy Change of combustion of methane from enthalpy of formation = -802.3 kJ mol^-1
\ No newline at end of file
diff --git a/3856/CH4/EX4.2/Ex4_2.sce b/3856/CH4/EX4.2/Ex4_2.sce
new file mode 100644
index 000000000..1ae4f6276
--- /dev/null
+++ b/3856/CH4/EX4.2/Ex4_2.sce
@@ -0,0 +1,23 @@
+//How high the person can climb on this energy intake

+

+//Example4.2

+

+clc;

+

+clear;

+

+M=73;  //Weight of the person in kg

+

+m=500;  //Mass of milk that person drink in g 

+

+Cv=720;  //Caloric value of milk in cal g^-1

+

+Mw=17;  //Percant of milk that converted in mechanical work

+

+W=(Mw*m*Cv*4.184)/100;  //Energy intake for mechanical work in J

+

+g=9.81;  //Acceleration due to gravity in m s^-2

+

+h=W/(M*g); //Person climb by this height in m

+

+printf("The person climbs to a height = %.1f*10^2 m",h*10^-2);

diff --git a/3856/CH4/EX4.2/Ex4_2.txt b/3856/CH4/EX4.2/Ex4_2.txt
new file mode 100644
index 000000000..09ed68f6e
--- /dev/null
+++ b/3856/CH4/EX4.2/Ex4_2.txt
@@ -0,0 +1 @@
+ The person climbs to a height = 3.6*10^2 m
\ No newline at end of file
diff --git a/3856/CH4/EX4.3/Ex4_3.sce b/3856/CH4/EX4.3/Ex4_3.sce
new file mode 100644
index 000000000..68096b6b5
--- /dev/null
+++ b/3856/CH4/EX4.3/Ex4_3.sce
@@ -0,0 +1,37 @@
+//Calculate the value of change in Internal energy and change in Enthalpy for the combution of Benzoic acid 

+

+//Example 4.3

+

+clc;

+

+clear;

+

+C=5267.8;  //Effective heat capcity of bomb calorimeter plus water im J K^-1

+

+T1=293.32;  //Initial temperature in K

+

+T2=295.37;  //Final temperature in K

+

+delT=T2-T1;  //Change in teperature in K

+

+M=122.12;  //Molar mass of Benzoic acid in g mol^-1

+

+m=0.4089;  //Mass of sample of Benzoic acid in g

+

+delU=-(C*delT*M)/(m*1000);  //Change in Enternal enegy in kJ mol^-1

+

+printf("Change in Enternal energy = %.0f kJ mol^-1",delU);(The answer vary due to round off error)

+

+R=8.314;  //Gas constant in J K^-1 mol^-1

+

+T=T1; //Temperature in K

+

+n1=7.5;  //Number of moles of gas for reactants

+

+n2=7;  //Number of mole of gas for product

+

+deln=n2-n1;  //Change of moles gas for reaction

+

+delH=delU+((R*T*deln)/1000); //Change in Enthalpy in kJ mol^-1

+

+printf("\nChange in Enthalpy = %.0f kJ mol^-1",delH); 

diff --git a/3856/CH4/EX4.3/Ex4_3.txt b/3856/CH4/EX4.3/Ex4_3.txt
new file mode 100644
index 000000000..e78d682c7
--- /dev/null
+++ b/3856/CH4/EX4.3/Ex4_3.txt
@@ -0,0 +1,2 @@
+ Change in Enternal energy = -3225 kJ mol^-1

+Change in Enthalpy = -3226 kJ mol^-1
\ No newline at end of file
diff --git a/3856/CH4/EX4.4/Ex4_4.sce b/3856/CH4/EX4.4/Ex4_4.sce
new file mode 100644
index 000000000..a3484850f
--- /dev/null
+++ b/3856/CH4/EX4.4/Ex4_4.sce
@@ -0,0 +1,27 @@
+//Compare the difference between change in Enthalpy and change in Enternal energy for 1 mol of ice melt  in to 1 mol of water at 273 K and one mole water change in to one mole steam at 373 K 

+

+//Example4.4

+

+clc;

+

+clear;

+

+Vbars=0.0196;  //Molar volume of ice in L mol^-1

+

+Vbarl=0.0180;  //Molar volume of water in L mol^-1

+

+P=1;  //Pressure in atm

+

+delV1=Vbarl-Vbars;  //Change in molar volume when water change in to steam in L mol^-1)

+

+E1=P*100*delV1;  //Differerce between change in Enthalpy and change in Enternal energy when ice melt in to water in J mol^-1 delH-delU 

+

+printf("(a)Difference between change in Enthalpy and change in Enternal energy for 1 mol of ice melt  in to 1 mol of water at 273 K = %.2f J mol^-1",E1);

+

+Vbarg=30.61;  //Molar volume of steam in L mol^-1

+

+delV2=Vbarg-Vbarl;  //Change in molar volume when water change in to steam in L mol^-1)

+

+E2=P*101.33*delV2;  //Differerce between change in Enthalpy and change in Enternal energy when water change in to steam delH-delU in J mol^-1

+

+printf("\n (b)Difference between change in Enthalpy and change in Enternal energy for one mole water change in to one mole steam at 373 K  = %.0f J mol^-1",E2);

diff --git a/3856/CH4/EX4.4/Ex4_4.txt b/3856/CH4/EX4.4/Ex4_4.txt
new file mode 100644
index 000000000..4a96d442d
--- /dev/null
+++ b/3856/CH4/EX4.4/Ex4_4.txt
@@ -0,0 +1,2 @@
+ (a)Difference between change in Enthalpy and change in Enternal energy for 1 mol of ice melt  in to 1 mol of water at 273 K = -0.16 J mol^-1

+ (b)Difference between change in Enthalpy and change in Enternal energy for one mole water change in to one mole steam at 373 K  = 3100 J mol^-1
\ No newline at end of file
diff --git a/3856/CH4/EX4.5/EX4_5.txt b/3856/CH4/EX4.5/EX4_5.txt
new file mode 100644
index 000000000..1d6bae5d2
--- /dev/null
+++ b/3856/CH4/EX4.5/EX4_5.txt
@@ -0,0 +1,2 @@
+ Change in Enternal energy = 526 J

+Change in Enthalpy = 877 J
\ No newline at end of file
diff --git a/3856/CH4/EX4.5/Ex4_5.sce b/3856/CH4/EX4.5/Ex4_5.sce
new file mode 100644
index 000000000..032b222db
--- /dev/null
+++ b/3856/CH4/EX4.5/Ex4_5.sce
@@ -0,0 +1,33 @@
+//Calculate the change in Enternal energy and change in Enthalpy for heating of Xenon 

+

+//Example4.5

+

+clc;

+

+clear;

+

+T1=300;  //Initial temperature in K

+

+T2=400;  //Final temperature in K

+

+m=55.40;  //Mass of Xenon in g

+

+M=131.29;  //Molecular mass of Xenon

+

+n=m/M;  //Number of mole of Xenon in mol

+

+R=8.314;  //Gas constant in J K^-1 mol^-1

+

+Cbarv=(3/2)*R;  //Molar constant volume in J K^-1 mol^-1

+

+delT=T2-T1;  //Thange in temperature in K

+

+delU=n*delT*Cbarv;  //Change in Enternal energy in J

+

+printf("Change in Enternal energy = %.0f J",delU);

+

+Cbarp=(5/2)*R;  //Molar constant pressure in J K^-1 mlo^-1

+

+delH=n*Cbarp*delT;  //Change in Enthalpy in J

+

+printf("\nChange in Enthalpy = %.0f J",delH);

diff --git a/3856/CH4/EX4.6/Ex4_6.sce b/3856/CH4/EX4.6/Ex4_6.sce
new file mode 100644
index 000000000..5d17e1375
--- /dev/null
+++ b/3856/CH4/EX4.6/Ex4_6.sce
@@ -0,0 +1,18 @@
+//Calculate the Enthalpy Change for heating of 1.46 moles of Oxygen

+

+//Example 4.6

+

+clc;

+

+clear;

+

+

+n=1.46;   //Number of moles of Oxygen

+

+function x=Cp(T) ,x=(25.7+0.0130*T), endfunction        //Molar Heat Capacity of Oxygen at Constant Pressure in J K^-1 mol^-1

+

+function y=f(T),y=n*Cp(T),endfunction             

+

+delH=intg(298,367,f);     //Enthalpy Change in J

+

+printf("Enthalpy Change = %.2f*10^3 J",delH*10^-3)

diff --git a/3856/CH4/EX4.6/Ex4_6.txt b/3856/CH4/EX4.6/Ex4_6.txt
new file mode 100644
index 000000000..6803fc0db
--- /dev/null
+++ b/3856/CH4/EX4.6/Ex4_6.txt
@@ -0,0 +1 @@
+ Enthalpy Change = 3.02*10^3 J
\ No newline at end of file
diff --git a/3856/CH4/EX4.7/Ex4_7.sce b/3856/CH4/EX4.7/Ex4_7.sce
new file mode 100644
index 000000000..0aaa6dc3e
--- /dev/null
+++ b/3856/CH4/EX4.7/Ex4_7.sce
@@ -0,0 +1,35 @@
+//Calculate the  work done if the expansion is carried out Adiabatically and Reversibly

+

+//Example 4.7

+

+clc;

+

+clear;

+

+n=0.850;  //Number of moles of momnoatomic ideal gas in mol

+

+R=0.08206;  //Gas constant in L atm K^-1

+

+T1=300;  //Initial temperature in K

+

+P1=15;  //Initial pressure in atm

+

+V1=(n*R*T1)/P1;  //Initial volume in L

+

+P2=1;  //Final pressure in atm

+

+gama=5/3; //Constant for Adiabatic Expansion

+

+V2=V1*(P1/P2)^(1/gama);  //Final volume in L

+

+T2=(P2*V2)/(n*R);  //Final temperature in K

+

+Cbarv=12.47;  //Molar consant volume heat capacity in J K^-1 mol^-1

+

+delU=n*Cbarv*(T2-T1);  //Change in Enternal energy in J 

+

+w=delU;  //Change in Enternal energy converted in to amount of work done in expansion is carried out Adiabatically and Reversibly in J

+

+printf("Work done = %.1f*10^3 J",w*10^-3);

+

+ 

diff --git a/3856/CH4/EX4.7/Ex4_7.txt b/3856/CH4/EX4.7/Ex4_7.txt
new file mode 100644
index 000000000..e0e9a5e96
--- /dev/null
+++ b/3856/CH4/EX4.7/Ex4_7.txt
@@ -0,0 +1 @@
+ Work done = -2.1*10^3 J
\ No newline at end of file
diff --git a/3856/CH4/EX4.8/Ex4_8.sce b/3856/CH4/EX4.8/Ex4_8.sce
new file mode 100644
index 000000000..e1438bc62
--- /dev/null
+++ b/3856/CH4/EX4.8/Ex4_8.sce
@@ -0,0 +1,19 @@
+//Calculate the standard molar Enthalpy of formatyion of Acetylene (C2H2) from its element

+

+//Example 4.8

+

+clc;

+

+clear;

+

+delH1deg=-393.5;  //Enthalpy change for the reaction C(graphite)+O2(g) givs CO2(g) in kJ mol^-1

+

+delH2deg=-285.8;  //Enthalpy change for the reaction H2(g)+1/2O2(g) givs H2O(l) in kJ mol^-1

+

+delH3deg=-2598.8;  //Enthalpy change for the reaction 2C2H2(g)+5O2(g)givs 4CO2(g)+2H2O(l)in kJ mol^-1

+

+delH4deg=-delH3deg;  //Enthalpy change for the reaction 4CO2(g)+2H2O(l)givs 2C2H2(g)+5O2(g)in kJ mol^-1

+

+delHdeg=(4*delH1deg+2*delH2deg+delH4deg)/2;  //Molar Enthalpy for formation of acetylene in kJ mol^-1

+

+printf("Molar Enthalpy = %.1f kJ mol^-1 ",delHdeg);  

diff --git a/3856/CH4/EX4.8/Ex4_8.txt b/3856/CH4/EX4.8/Ex4_8.txt
new file mode 100644
index 000000000..5b3ad1a95
--- /dev/null
+++ b/3856/CH4/EX4.8/Ex4_8.txt
@@ -0,0 +1 @@
+ Molar Enthalpy = 226.6 kJ mol^-1 
\ No newline at end of file
diff --git a/3856/CH4/EX4.9/Ex4_9.sce b/3856/CH4/EX4.9/Ex4_9.sce
new file mode 100644
index 000000000..467d6a390
--- /dev/null
+++ b/3856/CH4/EX4.9/Ex4_9.sce
@@ -0,0 +1,19 @@
+//Calulate the standard Enthalpy of the reaction C6H12O6(s)+6O2(g)givs 6CO2(g)+6H2O(l)at 298 K

+

+//Examlpe 4.9

+

+clc;

+

+clear;

+

+delfHbar1=-393.5;  //standard Molar Enthalpy of formation at 298 K and 1 Bar for CO2 in kJ mol^-1

+

+delfHbar2=-285.8;  //standard Molar Enthalpy of formation at 298 K and 1 Bar for H2O in kJ mol^-1

+

+delfHbar3=-1274.5;  //standard Molar Enthalpy of formation at 298 K and 1 Bar for C6H12O6 in kJ mol^-1

+

+delfHbar4=0;  //standard Molar Enthalpy of formation at 298 K and 1 Bar for O2 in kJ mol^-1

+

+delfHbar=(6*delfHbar1+6*delfHbar2)-(delfHbar3+6*delfHbar4);  //standard Enthalpy of the reaction in kJ mol^-1

+

+printf("Standard Enthalpy of the reaction = %.1f kJ mol^-1",delfHbar);

diff --git a/3856/CH4/EX4.9/Ex4_9.txt b/3856/CH4/EX4.9/Ex4_9.txt
new file mode 100644
index 000000000..9ca4955f4
--- /dev/null
+++ b/3856/CH4/EX4.9/Ex4_9.txt
@@ -0,0 +1 @@
+ Standard Enthalpy of the reaction = -2801.3 kJ mol^-1
\ No newline at end of file