Nitrogen combines with hydrogen to form ammonia. $\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)$ A reaction mixture containing $2.00$ mol of nitrogen, $6.00$ mol of hydrogen and $2.40$ mol of ammonia is left to attain equilibrium in a sealed vessel with a volume of $1\,\text{dm}^3$. It was determined that $2.32$ mol of nitrogen remained in the equilibrium mixture. Calculate the value of $K_c$.
- A$\dfrac{(1.76)^2}{(2.32)(6.96)^3}$
- B$\dfrac{(1.76)^2}{(2.32)(6.32)^3}$
- C$\dfrac{(2.08)^2}{(2.32)(6.32)^3}$
- D$\dfrac{(2.40)^2}{(2.32)(6.00)^3}$