Consider the oxidation of a generic metal MM into a metal oxide as shown in the reaction.

2M(s)+2O2(g) M2O4(s)

For this reaction, rxn=4.961 kJ/mol and rxn=12.12 J/(molK) at 298 K.

What is the standard change in Gibbs free energy for the reaction in the forward direction?

rxn= kJ/mol

What is the equilibrium constant of this reaction at 298 K?

P=

What is the equilibrium pressure of O2(g) over M(s) at 298 K?

O2= atm