9 files changed, 114 insertions, 0 deletions
diff --git a/3856/CH12/EX12.1/Ex12_1.jpg b/3856/CH12/EX12.1/Ex12_1.jpg
new file mode 100644
index 000000000..46f1e7fb1
--- /dev/null
+++ b/3856/CH12/EX12.1/Ex12_1.jpg
diff --git a/3856/CH12/EX12.1/Ex12_1.sce b/3856/CH12/EX12.1/Ex12_1.sce
new file mode 100644
index 000000000..f28db5d02
--- /dev/null
+++ b/3856/CH12/EX12.1/Ex12_1.sce
@@ -0,0 +1,32 @@
+//To Calculate the rate Constant for the Reaction
+
+//Example 12.1
+
+clc;
+clear;
+
+t=[0,2000,4000,6000,8000,10000,12000];//Time in seconds
+
+A=[1.5,1.26,1.07,0.92,0.81,0.72,0.65];//Absorbance
+
+A0=1.5;//Absorbance at t=0s
+
+Ainf=0.40;//Absorbance at t=infinity
+
+for i=1:6
+    x(i)=t(i);//Putting the x-axis as t/s
+end 
+
+for i=1:6
+    y(i)=log((A(i)-Ainf)/(A0-Ainf));//Putting the y-axis as ln((At-Ainf)/(A0-Ainf))
+end
+
+plot(x,y);//Plotting the Graph between x-axis and y-axis
+
+xlabel("t/s", "fontsize", 2);//Putting the x-axis as t/s
+
+ylabel("ln((At-Ainf)/(A0-Ainf))", "fontsize", 2);//Putting the y-axis as ln((At-Ainf)/(A0-Ainf))
+
+m=-(y(2)-y(1))/(x(2)-x(1));//Calculating the slope (Rate Constant of Reaction) of Graph
+
+printf("The rate constant for the reaction = %.3f*10^-4 s^-1",m*10^4);
diff --git a/3856/CH12/EX12.1/Ex12_1.txt b/3856/CH12/EX12.1/Ex12_1.txt
new file mode 100644
index 000000000..5aec91340
--- /dev/null
+++ b/3856/CH12/EX12.1/Ex12_1.txt
@@ -0,0 +1 @@
+ The rate constant for the reaction = 1.231*10^-4 s^-1
+\ No newline at end of file
diff --git a/3856/CH12/EX12.2/Ex12_2.sce b/3856/CH12/EX12.2/Ex12_2.sce
new file mode 100644
index 000000000..808255981
--- /dev/null
+++ b/3856/CH12/EX12.2/Ex12_2.sce
@@ -0,0 +1,33 @@
+//Calculate the standard molar  Enthalpy of activation (delH),standard molar Entropy of activation (delS)and Standard molar Gibbs energy of activation (delG) for the reaction CH3NC(g)=CH3CN(g)
+
+//Example 12.2
+
+clc;
+
+clear;
+
+k=4.0*10^13;  //Pre exponential factor in s^-1
+
+KB=1.381*10^-23;  //Boltzman constant in J K^-1
+
+h=6.626*10^-34;  //Planck's constant in J s
+
+R=8.314;  //Gas constant in J K^-1 mol^-1
+
+T=300;  //Absolute temperature in K
+
+e=2.718;  //ln constant
+  
+delS=log((k*h)/(e*KB*T))*R;  // Standard molar Entropy in J K^-1 mol^-1
+ 
+printf("Standard molar Entropy = %.2f J K^-1 mol^-1",delS);
+
+Ea=272;  //Activation Energy in kJ mol^-1
+
+delH=Ea-(R*T/1000);  //Standard molar Enthalpy in kJ mol^-1
+
+printf("\n Standard molar Enthalpy = %.0f kJ mol^-1",delH);
+
+delG=delH-(T*delS/1000);  //Standard molar Gibbs energy in kJ mol^-1(The answer vary due to round off error)
+
+printf("\n Standard molar Gibbs Energy = %.3f kJ mol^-1",delG);
diff --git a/3856/CH12/EX12.2/Ex12_2.txt b/3856/CH12/EX12.2/Ex12_2.txt
new file mode 100644
index 000000000..3d98b44fd
--- /dev/null
+++ b/3856/CH12/EX12.2/Ex12_2.txt
@@ -0,0 +1,3 @@
+ Standard molar Entropy = 7.12 J K^-1 mol^-1
+ Standard molar Enthalpy = 270 kJ mol^-1
+ Standard molar Gibbs Energy = 267.371 kJ mol^-1
+\ No newline at end of file
diff --git a/3856/CH12/EX12.3/Ex12_3.sce b/3856/CH12/EX12.3/Ex12_3.sce
new file mode 100644
index 000000000..974ad913e
--- /dev/null
+++ b/3856/CH12/EX12.3/Ex12_3.sce
@@ -0,0 +1,17 @@
+//Estimate the Rate constant for a diffusion controlled reaction in water
+
+//Example 12.3
+
+clc;
+
+clear;
+
+R=8.314;  //Gas constant in J K^-1 mol^-1
+
+T=298;  //Absolute temperature in K
+
+eta=8.9*10^-4;  //Viscosity of water in J s m^-3 (1J=1N m therefore N s m^-2=J s m^-3 )
+
+KD=(8*R*T)*1000/(3*eta);  //Rate constant for diffusion controlled reaction in M^-1 s^-1(1 m^3 mol^-1 s^-1=1000 M^-1 s^-1)
+
+printf("Rate constant for diffusion controlled reaction = %.1f*10^9 M^-1 s^-1",KD*10^-9);
diff --git a/3856/CH12/EX12.3/Ex12_3.txt b/3856/CH12/EX12.3/Ex12_3.txt
new file mode 100644
index 000000000..18c01d07e
--- /dev/null
+++ b/3856/CH12/EX12.3/Ex12_3.txt
@@ -0,0 +1 @@
+ Rate constant for diffusion controlled reaction = 7.4*10^9 M^-1 s^-1
+\ No newline at end of file
diff --git a/3856/CH12/EX12.4/Ex12_4.sce b/3856/CH12/EX12.4/Ex12_4.sce
new file mode 100644
index 000000000..a3f18e6f1
--- /dev/null
+++ b/3856/CH12/EX12.4/Ex12_4.sce
@@ -0,0 +1,25 @@
+//Calculate the Rate constant for Forward abd Reverse reaction 
+
+//Example 12.4
+
+clc;
+
+clear
+
+Tau=36*10^-6;  //The relaxation time for the system to reach the new equilibrium in s
+
+C1=1.0*10^-7; //Concentration of the Hydrogen ion in M
+
+C2=1.0*10^-7; //Concentration of the Hydroxyl ion in M (C1=C2)
+
+C3=55.5;  //Concentration of the Water in M 
+
+Kf=C3/((Tau)*((C1+C2)*(C3)+(C1*C2)));//Rate constant for Forward reaction in M^-1 s^-1(Kf*C1*C2=Kr*C3)(Tau=1/(Kf*(C1+C2)+Kr)
+
+printf("Rate constant for Forward reaction = %.1f*10^11 M^-1 s^-1",Kf*10^-11);
+
+K=(C1*C2)/C3; //Equilibrium Constant for the reaction in M (Hydrogen ion +Hydroxyl ion=Water )
+
+Kr=Kf*K; //Rate constant for Reverse reaction in s^-1
+
+printf("\n Rate constant for Reverse reaction = %.1f*10^-5 s^-1 ",Kr*10^5);
diff --git a/3856/CH12/EX12.4/Ex12_4.txt b/3856/CH12/EX12.4/Ex12_4.txt
new file mode 100644
index 000000000..cd7887a05
--- /dev/null
+++ b/3856/CH12/EX12.4/Ex12_4.txt
@@ -0,0 +1,2 @@
+ Rate constant for Forward reaction = 1.4*10^11 M^-1 s^-1
+ Rate constant for Reverse reaction = 2.5*10^-5 s^-1 
+\ No newline at end of file