State the definition of enthalpy change of neutralisation, $\Delta H_{\text{neut}}$.
Use equation 1 to work out the amount, in mol, of $\text{H}_2\text{SO}_4\text{(aq)}$ neutralised in the experiment.
Calculate $\Delta H_{\text{neut}}$ from the data in Table 2.1. Include units in your answer. Assume the specific heat capacity of the final solution is $4.18\,\text{J g}^{-1}\text{K}^{-1}$, that $1.00\,\text{cm}^3$ of the final solution has a mass of $1.00\,\text{g}$, that no heat is lost to the surroundings, that $\text{H}_2\text{SO}_4\text{(aq)}$ fully dissociates, and that the experiment is carried out at constant pressure. Show your working.
Complete the equation for the reaction when a solution of $\text{Ba(OH)}_2$ is added to aqueous sulfuric acid. Include state symbols.\n\n$\ldots\ldots\,\text{H}_2\text{SO}_4\text{(aq)} + \ldots\ldots\,\text{Ba(OH)}_2\text{(aq)} \rightarrow \ldots\ldots$
Explain why the enthalpy change of neutralisation cannot be found from adding dilute sulfuric acid to aqueous barium hydroxide.