Write an equation to represent phosphorus reacting with excess oxygen.
Describe how phosphorus(V) oxide reacts with water.
State the bonding and structure present in solid phosphorus(V) oxide.
Explain what is meant by the term weak Brønsted-Lowry acid.
Write an equation for $\text{SO}_2$ reacting with water.
$\text{SO}_2$ reacts with $\text{NO}_2$ in the atmosphere to make $\text{SO}_3$ and $\text{NO}$. $\text{NO}$ is then oxidised in air to produce $\text{NO}_2$. The reactions are: $\text{SO}_2 + \text{NO}_2 \rightarrow \text{SO}_3 + \text{NO}$ $2\text{NO} + \text{O}_2 \rightarrow 2\text{NO}_2$ State the function of $\text{NO}_2$ in this two-stage process.
Sulfur dioxide emissions from coal-fired power stations can be cut by adding powdered limestone to the coal. In reaction 1, limestone is heated to produce $\text{CaO}$. That 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 kind of reaction taking place in reaction 1.
Use the data to calculate the enthalpy change for reaction 2. $\Delta H_f$ values (kJ mol$^{-1}$): $\text{CaO}(s) = -635$, $\text{SO}_2(g) = -297$, $\text{CaSO}_4(s) = -1434$ Enthalpy change for reaction 2 = .......... $\text{kJ mol}^{-1}$.
Draw a dot-and-cross diagram for $\text{Cl}_2\text{O}$, showing only outer-shell electrons.
To prepare $\text{ClO}_2$, $\text{NaClO}_2$ is reacted with $\text{Cl}_2$. Write the oxidation state of chlorine in each species in the boxes provided. $2\text{NaClO}_2 + \text{Cl}_2 \rightarrow 2\text{ClO}_2 + 2\text{NaCl}$
$\text{Cl}_2\text{O}_6(g)$ is formed when $\text{ClO}_2(g)$ reacts with $\text{O}_3(g)$. $2\text{ClO}_2(g) + 2\text{O}_3(g) \rightleftharpoons \text{Cl}_2\text{O}_6(g) + 2\text{O}_2(g)$ $\Delta H = -216\,\text{kJ mol}^{-1}$ The reaction is carried out at $500\,\text{K}$ and $100\,\text{kPa}$. State and explain what happens to the yield of $\text{Cl}_2\text{O}_6(g)$ when the experiment is performed: • at $1000\,\text{K}$ and $100\,\text{kPa}$ • at $500\,\text{K}$ and $500\,\text{kPa}$
Suggest the bonding present in the oxide of E. Explain your answer.
Suggest the bonding present in the chloride of E. Explain your answer.