Identify that the equilibrium constant (Kc) indicates the relationship between product and reactant concentrations at equilibrium.

At $298 \text{ K}$, the system $\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g)$ reaches equilibrium. At equilibrium, $[\text{N}_2\text{O}_4] = 0.045 \text{ mol L}^{-1}$ and $[\text{NO}_2] = 0.062 \text{ mol L}^{-1}$. (a) Write the expression for the equilibrium constant, $K_c$, for this reaction. (1 mark) (b) Identify what the calculated value of $K_c$ indicates about the relative concentrations of reactants and products at equilibrium in this system. (1 mark)

For the reaction $$\text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g)$$ which statement correctly describes what the equilibrium constant $(K_c)$ represents?

For the equilibrium reaction \(\text{2NO}_{2}(g) \rightleftharpoons \text{N}_{2}\text{O}_{4}(g)\), the equilibrium constant expression is \(K_c = \frac{[\text{N}_{2}\text{O}_{4}]}{[\text{NO}_{2}]^{2}}\). Which statement correctly identifies what \(K_c\) indicates?