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+//Chapter-10,Example 8,Page 254
+clc();
+close();
+
+R=8.316    //gas constant
+
+F=96500    //Farade's constant
+
+n=2
+
+T=298      //temperature in Kelvin
+
+E0_Zn=-0.765   
+
+E0_Cu=0.337
+
+//cell reaction...Zn + Cu+2 <----> Zn+2 + Cu
+//  K = [Zn+2]*[Cu]/[Zn]*[Cu+2]...equilibrium constant
+
+E0_cell =E0_Cu - E0_Zn
+
+//at equilibrium two electrode potential s will be equal
+//   E0_cell = (2.303*R*T/n*F)*log10([Zn+2]*[Cu]/[Zn]*[Cu+2])
+//   E0_cell = (2.303*R*T/n*F)*log10(K)
+
+K = 10^(E0_cell/(2.303*R*T/(n*F)))
+
+printf('the equilibrium constant is K = ')
+
+disp(K)