$50\,\text{cm}^3$ of $1.0\,\text{mol dm}^{-3}$ $\text{H}_2\text{SO}_4$ is poured into $100\,\text{cm}^3$ of $1.0\,\text{mol dm}^{-3}$ NaOH in an insulated container. Before they are combined, both solutions are at $20\,^\circ\text{C}$. Once mixed, the temperature increases, and the maximum temperature reached is $29\,^\circ\text{C}$. Assume that: - every joule of energy released by the reaction is used to increase the temperature of the aqueous reaction mixture - the specific heat capacity of the mixture is $4.2\,\text{J cm}^{-3}\,\text{K}^{-1}$. What is the enthalpy of neutralisation value obtained from this experiment?
- A$-113.4\,\text{kJ mol}^{-1}$
- B$-56.7\,\text{kJ mol}^{-1}$
- C$-37.8\,\text{kJ mol}^{-1}$
- D$-18.9\,\text{kJ mol}^{-1}$