Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.

M2O(s) 2M(s)+12O2(g)M2O(s) 2M(s)+12O2(g)

What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?

Substance	Gf(kJ/mol)
M2O(s)	6.90
M(s)	0
O2(g)	0

rxn= kJ/molkJ/mol

What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?

=

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

O2= atm