Part 1) We're being asked to calculate the standard change in Gibbs energy for the reaction.

**M _{2}O_{3}(s) ⇌ 2 M(s) + 3/2 O_{2}(g)**

We can use the following equation to solve for ** ΔG˚_{rxn}**:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

The values for **ΔG˚ _{f}**:

ΔG˚_{f}, M_{2}O_{3}(s) = –8.00 kJ/mol

ΔG˚_{f}, M(s) = 0 kJ/mol

ΔG˚_{f}, O_{2}(g) = 0 kJ/mol

Note that we need to *multiply each ΔG˚ _{f} by the stoichiometric coefficient* since ΔG˚

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

**M _{2}O_{3}(s) ⇌ 2 M(s) + 3/2 O_{2}(g)**

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

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

What is the equilibrium pressure of O_{2}(g) over M(s) at 298 K?

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