For a reaction $2\mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}, {\mathrm{K}}_{\mathrm{c}}$ is $2\times {10}^{-3}.$ At a given time, the reaction mixture has $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3\times {10}^{-4}\mathrm{M}.$ Which of the following options is correct?

If the value of reaction quotient (Q) is higher than that of equilibrium constant (K), the reaction favour reactants more since the amount of products in the system is higher than that of reactants. Then the reaction tends to form more reactants in order to keep the equilibrium at constant.

If Q is lower than K, the system is composed of more reactants than products. Therefore, the reaction tends to form more products in order to keep the equilibrium.

If Q and K are equal, then the reaction mixture is at an equilibrium.

$\mathrm{Q} = \frac{\left[\mathrm{B}\right]\left[\mathrm{C}\right]}{{\left[\mathrm{A}\right]}^2} = \frac{3\times {10}^{-4} \times 3\times {10}^{-4}}{{\left(3\times {10}^{-4}\right)}^2} = 1 > {\mathrm{K}}_{\mathrm{C}}$

So, Reaction will proceeds to the left.