For the reaction F₂(g) 2F(g)
At a particular temperature, the concentrations at equilibrium were observed to be [F₂] = 2.0 *10^-² mol/L and [F] = 2.0 * 10^-⁴ mol/L. Calculate the value of the equilibrium constant from these data. (The units are deleted.)

Question

For the reaction F₂(g)

For the reaction F<sub>2</sub>(g) 2F(g) At a particular temperature, the concentrations at equilibrium were observed to be [F<sub>2</sub>] = 2.0 *10<sup>-</sup><sup>2</sup> mol/L and [F] = 2.0 * 10<sup>-</sup><sup>4</sup> mol/L. Calculate the value of the equilibrium constant from these data. (The units are deleted.) A) B) 1.7 C) 5.0 * 10<sup>5</sup> D) 2.0 * 10<sup>-</sup><sup>6</sup> E) none of these

2F(g)
At a particular temperature, the concentrations at equilibrium were observed to be [F₂] = 2.0 *10^-² mol/L and [F] = 2.0 * 10^-⁴ mol/L. Calculate the value of the equilibrium constant from these data. (The units are deleted.)

Quizplus · Accepted Answer

The equilibrium constant expression for the given reaction is Kc = [F]^2/[F₂]. Substituting the given values, we get Kc = (2.0)^2/(2.0) = 2.0 x 10^1-2 = 2.0 x 10^-2. Therefore, the correct answer is D, 2.0 x 10^-2.

For the Reaction F2(g) 2F(g)

For the Reaction F₂(g) 2F(g)