Draw a diagram showing the shape of each oxide molecule, $\text{SO}_3$ and $\text{Cl}_2\text{O}$. Name each shape. In $\text{SO}_3$, each oxygen atom is double-bonded to the sulfur atom.
Explain why $\text{MgO}$ has a higher melting point than $\text{Na}_2\text{O}$.
Explain why the melting point of $\text{SiO}_2$ is much higher than that of $\text{SO}_3$.
$\text{SO}_3$ is formed when $\text{SO}_2$ reacts with $\text{O}_2$ in the Contact process. A dynamic equilibrium is reached. $2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) \quad \Delta H = -196\,\text{kJ mol}^{-1}$
Explain why raising the total pressure, at constant temperature, increases the rate at which $\text{SO}_3$ is produced and also increases the yield of $\text{SO}_3$.
Explain why the slopes of the $\text{SO}_2$ and $\text{O}_2$ lines get smaller with time.
Explain why all three lines level off.
Suggest a reason why the initial gradient for the $\text{SO}_2$ line is steeper than for the $\text{O}_2$ line.
A mixture containing $2.00$ moles of $\text{SO}_2(g)$ and $2.00$ moles of $\text{O}_2(g)$ is sealed in a container with a suitable catalyst, at constant temperature and pressure. At equilibrium, the mixture contains $1.98$ moles of $\text{SO}_3(g)$. The total volume of the equilibrium mixture is $40.0\,\text{dm}^3$. $2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)$
Write the expression for the equilibrium constant, $K_c$, for the reaction in which $\text{SO}_2(g)$ and $\text{O}_2(g)$ form $\text{SO}_3(g)$.
Calculate the amount, in moles, of $\text{SO}_2(g)$ and $\text{O}_2(g)$ present in the equilibrium mixture.
Use your answers to d(i) and d(ii) to work out the value of $K_c$ for this equilibrium mixture. State the units of $K_c$.