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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);
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