The decomposition of nitrogen dioxide on heating is represented by the equation below. $2\text{NO}_2(g) \rightleftharpoons 2\text{NO}(g) + \text{O}_2(g)$. If $4\text{ mol}$ of nitrogen dioxide are introduced into a $1\text{ dm}^3$ vessel and the mixture is allowed to reach a steady temperature, the equilibrium mixture contains $0.8\text{ mol}$ of oxygen. Determine the equilibrium constant, $K_c$, at the temperature used in the experiment.
- A$\frac{0.8^2 \times 0.8}{4^2}$
- B$\frac{1.6 \times 0.8}{2.4^2}$
- C$\frac{1.6^2 \times 0.8}{4^2}$
- D$\frac{1.6^2 \times 0.8}{2.4^2}$