From the given thermochemical data: O(g) + e- → O-(g) ; ΔH = -141.4 kJ mol-1 O-(g) + e- → O2-(g) ; ΔH = +790.8 kJ mol-1 Calculate the total energy change for the production of O2-(g) from O(g).

For a spontaneous process occurring at constant temperature and pressure, the changes in Gibbs free energy (ΔG) and entropy (ΔS) satisfy:

For a phase reaction A ⇌ B, the standard Gibbs free energy change is given by ΔG° = 105 - 35 log10 T (in J mol-1). Find the transition temperature (in °C) of the reaction at 1 bar pressure.