Question

Consider the following equilibrium:

Answer 1

Answer:

A) is true

Explanation:

For the reaction:

O₂(g) + 2F₂(g) ⇄ 2OF₂(g); Kp = 2,3x10⁻¹⁵

kp is defined as:

Kp = 2,3x10⁻¹⁵ = [OF₂]²/[O₂] [F₂]²

A) If the reaction mixture initially contains only OF₂(g), then at equilibrium, the  reaction mixture will consist of essentially only O₂(g) and F₂(g).  TRUE. As the kp is 2,3x10⁻¹⁵ means per 1 of [O₂] [F₂]² you will have just 2,3x10⁻¹⁵ of [OF₂]²

B) For this equilibrium, Kc = Kp.  FALSE. That is true just when moles of reactants are the same than moles of products. Here there are 3 moles of reactants vs 2 moles of products.

C) If the reaction mixture initially contains only OF₂(g), then the total pressure at  equilibrium will be less than the total initial pressure.  FALSE. Because per 2 moles of OF₂(g) you will produce 3 moles of gas increasing pressure.

D) If the reaction mixture initially contains only O₂(g) and F₂(g), then at equilibrium,  the reaction mixture will consist of essentially only OF₂(g).  FALSE. For the same reason of A), the mixture will contains essentially only O₂(g) and F₂(g)

E) If the reaction mixture initially contains only O₂(g) and F₂(g), then the total  pressure at equilibrium will be greater than the total initial pressure. FALSE. If mixture initially contains only O₂(g) and F₂(g), 3 moles will of gas will react to produce 2 moles of gas doing pressure decreases.

I hope it helps!