Chemistry Gibbs Free Energy Solution: Consider the decomposition of a metal oxide to its...

🤓 Based on our data, we think this question is relevant for Professor Mcafee's class at UNT.

Solution: Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.                                     M    3O4 (s) ⇌ 3 M (s) + 2 O2 (g) i) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?ii) What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?iii) What is the equilibrium pressure of O2 (g) over M (s) at 298 K? 

Problem

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

                                     M    3O(s) ⇌ 3 M (s) + 2 O(g) 

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

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

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

Solution

i)

$ΔG^o_{rxn} = products - reactants$

$ΔG^o_{rxn} = [(3 mole M)(0 kJ/mol) + (2 mol O2)(0 kJ/mol)] - [(1 mole M_3O_4)(-9.50 kJ/mol)] = 9.50 kJ$

Solution BlurView Complete Written Solution