$50\ \text{cm}^3$ of $2.50\ \text{mol dm}^{-3}$ hydrochloric acid was poured into a polystyrene beaker with negligible heat capacity. Its temperature was measured, after which $50\ \text{cm}^3$ of $2.50\ \text{mol dm}^{-3}$ NaOH at the same temperature was added rapidly, with stirring. The temperature increased by $17\ ^\circ\text{C}$. For the purposes of the calculation, the final solution can be treated as having a specific heat capacity of $4.2\ \text{J g}^{-1}\ \text{K}^{-1}$. What approximate value would you obtain for the molar enthalpy change of neutralisation of hydrochloric acid and sodium hydroxide from this experiment?
- A$-\dfrac{50 \times 4.2 \times 17}{0.050 \times 2.5}\ \text{J mol}^{-1}$
- B$-\dfrac{50 \times 4.2 \times 17}{0.10 \times 2.5}\ \text{J mol}^{-1}$
- C$-\dfrac{100 \times 4.2 \times 17}{0.050 \times 2.5}\ \text{J mol}^{-1}$
- D$-\dfrac{100 \times 4.2 \times 17}{50 \times 2.5}\ \text{J mol}^{-1}$