Question

Calculate the Gibbs free energy change for the following reaction at 298 K: 2H2(g) + O2(g) → 2H2O(l) Given, ΔH = -483.6 kJ/mol and ΔS = -109.4 J/K/mol.

Answer 1

To calculate the Gibbs free energy change  G  for the reaction, we can use the following equation:G = H - TSwhere H is the change in enthalpy, T is the temperature in Kelvin, and S is the change in entropy.Given values:H = -483.6 kJ/molS = -109.4 J/K/molT = 298 KFirst, we need to convert S to kJ/K/mol:S = -109.4 J/K/mol   1 kJ / 1000 J  = -0.1094 kJ/K/molNow, we can plug the values into the equation:G =  -483.6 kJ/mol  -  298 K  -0.1094 kJ/K/mol G = -483.6 kJ/mol + 32.6 kJ/molG = -451 kJ/molSo, the Gibbs free energy change for the reaction is -451 kJ/mol.