Answer :
Final answer:
The question is about chemical equilibrium in the given reaction. The equilibrium constant K is provided, and the initial and equilibrium concentrations of the species are known. We can calculate the equilibrium concentration of HF by plugging the known values into the equilibrium equation and solving for HF.
Explanation:
In this scenario, we're looking at the concept of chemical equilibrium in a reaction. The provided equilibrium constant (K) is given as 46.5, which allows us to calculate the concentrations of the components at equilibrium. Initially, we have 0.5 moles of HF in a 1 liter flask, which implies an initial HF concentration of 0.5 moles/L, before equilibrium is reached.
The reaction given is 2 HF(g) → H₂(g) + F₂(g), in which HF splits into H₂ and F₂. Given that we know the concentrations of H₂ and F₂ at equilibrium are 0.75 moles/L each, we can use the expression K = [H₂][F₂] / [HF]² to find the concentration of HF at equilibrium.
Plugging in the known values and solving for [HF] will yield the equilibrium concentration for HF.
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