Calculate equilibrium constants (Kc) and the concentrations of reactants and products. Assume [reactants]initial = [reactants]equilibrium when 𝐾c is very small and state assumption when used. (Formula: 𝐾c = [C]c[D]d [A]a[B]b for the reaction aA + bB ⇋ cC + dD) Chem istry 2025 v1.3

The decomposition of dinitrogen tetroxide is represented by the equation: $$\mathrm{N_2O_4(g) \rightleftharpoons 2NO_2(g)}$$ At equilibrium at 25 °C, the concentration of $\mathrm{N_2O_4}$ is $0.048 \text{ mol L}^{-1}$ and the concentration of $\mathrm{NO_2}$ is $0.064 \text{ mol L}^{-1}$. Calculate the equilibrium constant, $K_c$, for this reaction. Show your working.

For the equilibrium: $2\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g)$, the equilibrium concentrations at 298 K are: $[\text{NO}_2] = 0.042 \text{ mol L}^{-1}$ and $[\text{N}_2\text{O}_4] = 0.028 \text{ mol L}^{-1}$. Calculate the equilibrium constant $K_c$ for this reaction.

Calculate the equilibrium constant (K_c) for the decomposition reaction at this temperature.

At 298 K, nitrogen dioxide (NO₂) exists in equilibrium with dinitrogen tetroxide (N₂O₄). The equilibrium is represented by: $$2\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g)$$ At equilibrium at 298 K, the concentrations are: $[\text{NO}_2] = 0.045 \text{ mol L}^{-1}$ and $[\text{N}_2\text{O}_4] = 0.28 \text{ mol L}^{-1}$ Calculate the equilibrium constant, $K_c$, for this reaction at 298 K. Show your working.