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diff --git a/884/CH19/EX19.3/Example19_3.sce b/884/CH19/EX19.3/Example19_3.sce
new file mode 100755
index 000000000..d61d9a19d
--- /dev/null
+++ b/884/CH19/EX19.3/Example19_3.sce
@@ -0,0 +1,15 @@
+//computation of standard emf of a cell

+

+clear;

+clc;

+

+printf("\t Example 19.3\n");

+

+E0cathode=0.8;//standard electrode potential of cathode(Ag+/Ag), V

+E0anode=-2.37;//standard electrode potential of anode(Mg2+/Mg), V

+

+E0cell=E0cathode-E0anode;//standard emf of the cell, V

+

+printf("\t the standard emf of the cell is : %4.2f V\n",E0cell);

+

+//End

diff --git a/884/CH19/EX19.4/Example19_4.sce b/884/CH19/EX19.4/Example19_4.sce
new file mode 100755
index 000000000..262d00c05
--- /dev/null
+++ b/884/CH19/EX19.4/Example19_4.sce
@@ -0,0 +1,18 @@
+//computation of equilibrium constant for a reaction

+

+clear;

+clc;

+

+printf("\t Example 19.4\n");

+

+n=2;

+E0cathode=0.15;//standard electrode potential of cathode(Cu2+/Cu+), V

+E0anode=-0.14;//standard electrode potential of anode(Sn2+/Sn), V

+

+E0cell=E0cathode-E0anode;//standard emf of the cell, V

+

+K=exp(n*E0cell/0.0257);//equilibrium constant, from the formula E0cell=0.0257*lnK/n

+

+printf("\t the equilibrium constant for the given reaction is : %4.2f*10^9\n",K*10^-9);

+

+//End

diff --git a/884/CH19/EX19.5/Example19_5.sce b/884/CH19/EX19.5/Example19_5.sce
new file mode 100755
index 000000000..3843ec075
--- /dev/null
+++ b/884/CH19/EX19.5/Example19_5.sce
@@ -0,0 +1,20 @@
+//computation of standard free energy change for a reaction

+

+clear;

+clc;

+

+printf("\t Example 19.5\n");

+

+n=6;

+F=96500;//faraday constant, J/V mol

+

+E0cathode=-2.87;//standard electrode potential of cathode(Ca2+/Ca), V

+E0anode=1.5;//standard electrode potential of anode(Au3+/Au), V

+

+E0cell=E0cathode-E0anode;//standard emf of the cell, V

+

+deltaG0=-n*F*E0cell;//standard free energy change for the reaction, kJ/mol

+

+printf("\t the standard free energy change for the reaction is : %4.2f*10^3 kJ/mol \n",deltaG0*10^-6);

+

+//End

diff --git a/884/CH19/EX19.6/Example19_6.sce b/884/CH19/EX19.6/Example19_6.sce
new file mode 100755
index 000000000..c1b322247
--- /dev/null
+++ b/884/CH19/EX19.6/Example19_6.sce
@@ -0,0 +1,27 @@
+//computation of standard free energy change for a reaction

+

+clear;

+clc;

+

+printf("\t Example 19.6\n");

+

+n=2;

+F=96500;//faraday constant, J/V mol

+

+Co2=0.15;//conc of Co2+ ions, M

+Fe2=0.68;//conc of Fe2+ ions, M

+

+E0cathode=-0.44;//standard electrode potential of cathode(Fe2+/Fe), V

+E0anode=-0.28;//standard electrode potential of anode(Co2+/Co), V

+

+E0cell=E0cathode-E0anode;//standard emf of the cell, V

+

+Ecell=E0cell-0.0257/2*log(Co2/Fe2);//calculation of cell potential at non standard conditions, V

+

+if(Ecell>0) then

+    printf("\t the reaction would proceed spontaneously in the direction written \n");

+else

+    printf("\t the reaction is not spontaneously in the direction written \n");

+    end;

+

+//End

diff --git a/884/CH19/EX19.7/Example19_7.sce b/884/CH19/EX19.7/Example19_7.sce
new file mode 100755
index 000000000..86597ce70
--- /dev/null
+++ b/884/CH19/EX19.7/Example19_7.sce
@@ -0,0 +1,23 @@
+//computation of concentration of component from cell potential

+

+clear;

+clc;

+

+printf("\t Example 19.7\n");

+

+n=2;

+

+Zn=1;//conc of Zn2+ ions, M

+pH2=1;//pressure of H2 gas, atm

+

+Ecell=0.54;//emf of the cell, V

+

+E0cell=0.76;//standard emf of the cell, V

+

+Q=exp(-(Ecell-E0cell)*2/0.0257);//since Ecell=E0cell-0.0257/2*log(Q) where Q=(Zn2+)*pH2/(H+)^2

+

+H=sqrt(Zn*pH2/Q);//the conc of H+ ions, M

+

+printf("\t the molar concentration of H+ ion is : %2.0f*10^-4 M \n",H*10^4);

+

+//End

diff --git a/884/CH19/EX19.9/Example19_9.sce b/884/CH19/EX19.9/Example19_9.sce
new file mode 100755
index 000000000..07527a10c
--- /dev/null
+++ b/884/CH19/EX19.9/Example19_9.sce
@@ -0,0 +1,24 @@
+//quantitative aspects of electrolysis

+

+clear;

+clc;

+

+printf("\t Example 19.9\n");

+

+t=7.44*3600;//time, sec

+A=1.26;//current in ampere

+q=A*t;//charge passed, coulomb

+F=96500;//faraday constant, J/V mol

+ne=q/F;//moles of electrons

+nO2=ne/4;//moles of oxygen

+nH2=ne/2;//moles of H2

+

+R=0.0821;//gas constant, L atm/K

+T=273;//temperature in Kelvin

+P=1;//pressure in atm

+VO2=nO2*R*T/P;//volume of oxygen gas generated

+VH2=nH2*R*T/P;//volume of H2 gas generated

+

+printf("\t the volume of O2 gas and H2 gas generated are : %4.2f L and %4.2f L respectively\n",VO2,VH2);

+

+//End