State the effect of a catalyst on a reaction. Explain how a catalyst produces this effect.
State what the term heterogeneous means when applied to catalysts.
The following bond energies are provided: $\text{S} = \text{O}$ (in $\text{SO}_2$): $534\,\text{kJ mol}^{-1}$ $\text{O} = \text{O}$: $496\,\text{kJ mol}^{-1}$ Using these data, together with the enthalpy change for the conversion of sulfur dioxide into sulfur trioxide, calculate the $\text{S} = \text{O}$ bond energy in $\text{SO}_3$.
A reaction pathway diagram for both the catalysed and uncatalysed reactions between $\text{SO}_2$ and $\text{O}_2$ is shown. The letters A-E stand for energy changes. Complete the table by saying which letter, A-E, shows: • the energy change for the production of $\text{SO}_3$ • the activation energy for the production of $\text{SO}_3$ without a catalyst • the activation energy for the first step in the decomposition of $\text{SO}_3$ in the presence of a catalyst
State and explain what happens to the rate of production of $\text{SO}_3$ when temperature is increased.
State and explain the effect of increasing temperature on the yield of $\text{SO}_3$.
The $\text{SO}_3$ made is changed into sulfuric acid in two stages. In the first stage, the $\text{SO}_3$ is reacted with concentrated sulfuric acid to make oleum, $\text{H}_2\text{S}_2\text{O}_7$. The oleum is then reacted with water to produce sulfuric acid. Suggest an equation for the reaction of oleum, $\text{H}_2\text{S}_2\text{O}_7$, with water to form sulfuric acid.
Complete the ‘dot-and-cross’ diagram so that it shows the bonding in one $\text{SO}_2$ molecule. Show only outer electrons.
State what is meant by the term strong Brønsted-Lowry acid.
Write an equation showing the acid-base behaviour of sulfuric acid in water. Include state symbols.