At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10².
H₂(g) + F₂(g) 2HF(g)
If 1.00 mol of each of H₂ and F₂ are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H₂ and HF.

Question

At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10².
H₂(g) + F₂(g)

At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10<sup>2</sup>. H<sub>2</sub>(g) + F<sub>2</sub>(g) 2HF(g) If 1.00 mol of each of H<sub>2</sub> and F<sub>2</sub> are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H<sub>2</sub> and HF.

2HF(g)
If 1.00 mol of each of H₂ and F₂ are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H₂ and HF.

Quizplus · Accepted Answer

The Answer of At a high temperature, the following reaction has an equilibrium constant of 1.0 × 10². H₂(g) + F₂(g) 2HF(g) If 1.00 mol of each of H₂ and F₂ are allowed to come to equilibrium in a 10.0 L vessel, calculate the equilibrium amounts of H₂ and HF.

At a High Temperature, the Following Reaction Has an Equilibrium