Estimate ΔG°rxn for the following reaction at 449.0 K. CH2O (g) + 2 H2 (g) → CH4 (g) + H2O (g) ΔH° = - 94.9 kJ; ΔS° = - 224.2 J/K

This equation relates all three variables, so just plug in all of the given values. Don't forget to convert deltaS into kJ/K because Gibbs free energy is measured in kJ. The K used in temperature cancels out the K in kJ/K, leaving only kJ as your units. Don't forget sig figs!