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+//Calculate the Equilibrium constant for the reaction 2H2(g)+O2(g)=2H2O(l)
+
+//Example 9.3
+
+clc;
+
+clear;
+
+delG1=-237.2; //Standard Gibbs enaergy for H2O in kJ mol^-1
+
+delG2=0; //Standard Gibbs enaergy for H2 in kJ mol^-1
+
+delG3=0;  //Standard Gibbs enaergy for O2 in kJ mol^-1
+
+delG=2*delG1-2*delG2-delG3; //Standard Gibbs enaergy change for the reaction in kJ mol^-1
+
+R=8.314;  //Gas constant in J K^-1 mol^-1
+
+T=298;   //Temperature in K
+
+Kp=exp(-(delG*1000)/(R*T));  //Equilibrium constant 
+
+printf("Equilibrium constant = %.1f*10^83",Kp*10^-83); 
+