When phosphorus reacts with excess oxygen, phosphorus(V) oxide is formed. Write an equation that represents phosphorus reacting with excess oxygen.
Describe how phosphorus(V) oxide reacts with water.
State the structure and bonding present in solid phosphorus(V) oxide.
The two main oxides of sulfur are $\text{SO}_2$ and $\text{SO}_3$. When $\text{SO}_2$ dissolves in water, only a small fraction reacts with the water to produce a weak Brønsted-Lowry acid. Explain what is meant by the term weak Brønsted-Lowry acid.
Write the equation for the reaction between $\text{SO}_2$ and water.
$\text{SO}_2$ reacts with $\text{NO}_2$ in the atmosphere to form $\text{SO}_3$ and NO. NO is then oxidised in air to form $\text{NO}_2$. $\text{SO}_2 + \text{NO}_2 \rightarrow \text{SO}_3 + \text{NO}$ $2\text{NO} + \text{O}_2 \rightarrow 2\text{NO}_2$ State the role of $\text{NO}_2$ in this two-stage process.
Emissions of $\text{SO}_2$ from coal-fired power stations can be lowered by mixing the coal with powdered limestone. Limestone is heated so that CaO is made in reaction 1. This then reacts with $\text{SO}_2$ and $\text{O}_2$ to form $\text{CaSO}_4$ in reaction 2. reaction 1: $\text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g)$ reaction 2: $\text{CaO}(s) + \text{SO}_2(g) + \tfrac{1}{2}\text{O}_2(g) \rightarrow \text{CaSO}_4(s)$ State the type of reaction occurring in reaction 1.
Using the data below, calculate the enthalpy change for reaction 2. $\Delta H_f / \text{kJ mol}^{-1}$: $\text{CaO}(s) = -635$, $\text{SO}_2(g) = -297$, $\text{CaSO}_4(s) = -1434$.
Draw a ‘dot-and-cross’ diagram of $\text{Cl}_2\text{O}$. Include only the outer-shell electrons.
Write the oxidation state of chlorine in each species in the boxes provided. $\text{2NaClO}_2 + \text{Cl}_2 \rightarrow 2\text{ClO}_2 + 2\text{NaCl}$
$\text{Cl}_2\text{O}_6(g)$ is made by reacting $\text{ClO}_2(g)$ with $\text{O}_3(g)$. $2\text{ClO}_2(g) + 2\text{O}_3(g) \rightleftharpoons \text{Cl}_2\text{O}_6(g) + 2\text{O}_2(g) \qquad \Delta H = -216\,\text{kJ mol}^{-1}$ The reaction is carried out at $500\,\text{K}$ and $100\,\text{kPa}$. State and explain the effect on the yield of $\text{Cl}_2\text{O}_6(g)$ when the experiment is carried out: • at $1000\,\text{K}$ and $100\,\text{kPa}$ • at $500\,\text{K}$ and $500\,\text{kPa}$
Suggest the type of bonding shown by the oxide of E. Explain your answer.
Suggest the type of bonding shown by the chloride of E. Explain your answer.