1. The problem statement, all variables and given/known data Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g) ΔHorxn=55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 370K ? Assume that the initial pressure of N2O4 is the same (0.100 atm). How is this problem done? We know: Delta H of reaction = 55.3 kJ Equilibrium means Delta G = 0 AT 298 K and 58% decomposition. We need to find what percentage of N2O4 decomposes at 370K. I'm not entirely sure what equations I should be using. We are talking about Gibbs Free Energy. This is a mast. chem. problem and the last of the 40-50 I have left. If someone could guide me towards a correct equation, I can work this out.