Question

When the oxide of generic metal M is heated at 25.0 ∘ C , a negligible amount of M is produced. MO 2 ( s ) − ⇀ ↽ − M ( s ) + O 2 ( g ) Δ G ∘ = 290.2 kJ mol
1. When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C ( s ).
2. What is the thermodynamic equilibrium constant for the coupled reaction?K = ????

Answer 1

Answer:

1. C(s) + O₂(g) ⇄ CO₂(g)

2. $K=\frac{[CO_{2}]}{[O_{2}]}$

Explanation:

When the oxide of generic metal M is heated at 25.0 °C, a negligible amount of M is produced. MO₂( s ) ⇄ M(s) + O₂(g) ΔG° = 290.2 kJ/mol.

1. When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s).

The chemical equation for the coupled reaction is:

C(s) + O₂(g) ⇄ CO₂(g)

2. What is the thermodynamic equilibrium constant for the coupled reaction?

The thermodynamic equilibrium constant (K) is the product of the concentration of the products raised to their stoichiometric coefficients divided by the product of the concentration of the reactants raised to their stoichiometric coefficients. Only gases and aqueous species are included.

$K=\frac{[CO_{2}]}{[O_{2}]}$