The enthalpy change of neutralisation for $\text{HNO}_3(aq)$ reacting with $\text{NaOH}(aq)$ is $-57.0\ \text{kJ mol}^{-1}$. During an experiment, $20.0\ \text{cm}^3$ of $4.00\ \text{mol dm}^{-3}\ \text{HNO}_3$ is combined with $30.0\ \text{cm}^3$ of $2.00\ \text{mol dm}^{-3}\ \text{NaOH}$ in an insulated container. Both solutions begin at $25.0\ ^\circ\text{C}$. You may assume that the heat capacity of the product mixture is $4.2\ \text{J cm}^{-3}\ ^\circ\text{C}^{-1}$ and that no heat is lost. What is the highest final temperature reached by the mixture?
- A$41.3\ ^\circ\text{C}$
- B$44.0\ ^\circ\text{C}$
- C$46.7\ ^\circ\text{C}$
- D$52.1\ ^\circ\text{C}$