Consider the reaction.

$2 HF(g) \longleftrightarrow H_2(g)+F_2(g)$



At equilibrium at 600 K, the concentrations are as follows:

$\begin{array}{l}

{[HF]=5.82 \times 10^{-2} M} \\

{\left[H_2\right]=8.4 \times 10^{-3} M} \\

{\left[F_2\right]=8.4 \times 10^{-3} M}

\end{array}$



What is the value of $K_{eq}$ for the reaction expressed in scientific notation?

A$1.2 \times 10^{-3}$

B$2.1 \times 10^{-2}$

C$2.1 \times 10^2$

D$1.2 \times 10^3$