Add labelled arrows to the energy profile to show the reaction enthalpy, $\Delta H$, and the activation energy for the forward reaction, $E_a$.
$0.0500\,\text{mol}$ of $\text{N}_2\text{O}_4$ was put into a sealed vessel with volume $1.00\,\text{dm}^3$, at $50^{\circ}\text{C}$ and pressure $1.68 \times 10^5\,\text{Pa}$. The mass of the equilibrium mixture produced was $4.606\,\text{g}$. Calculate the average molecular mass, $M_r$, of the equilibrium mixture produced. Give your answer to three significant figures.
Let the number of moles of $\text{N}_2\text{O}_4$ that dissociated be $n$. State, in terms of $n$, the amount, in moles, of $\text{NO}_2$ present in the equilibrium mixture.
The amount of $\text{N}_2\text{O}_4$ left at equilibrium is $(0.05 - n)$. State, in terms of $n$, the total amount, in moles, of gas present in the equilibrium mixture.
State, in terms of $n$, the mole fraction for $\text{NO}_2$ in the equilibrium mixture.
For this equilibrium mixture, the mole fraction of $\text{NO}_2$ is $0.400$. Use your answers to (ii) and (iv) to find the amount in moles of each gas in the equilibrium mixture. Give your answers to three significant figures.
Write the expression for the equilibrium constant, $K_p$, for this system.
Using the total pressure of the mixture, $1.68 \times 10^5\,\text{Pa}$, calculate the value of the equilibrium constant, $K_p$, and include its units.