Equilibrium constant, $K_c$ for the reaction $\mathrm{N}_{2(g)} + 3\mathrm{H}_{2(g)}$ ⇌ $2\mathrm{NH}_{3(g)}$ at 500 K is 0.061. At a particular time, the analysis shows that composition of the reaction mixture is 3.0 $\text{mol L}^{-1} \mathrm{N}_2$, 2.0 $\text{mol L}^{-1} \mathrm{H}_2$ and 0.5 $\text{mol L}^{-1} \mathrm{NH}_3$. Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?