A student conducts two separate calorimetry trials to investigate the enthalpy of neutralization for the reaction represented by the equation below:

\[ \text{HCl(aq)} + \text{NaOH(aq)} \rightarrow \text{NaCl(aq)} + \text{H}_2\text{O(l)} \quad \Delta H^\circ_{\text{rxn}} = -56\text{ kJ/mol}_{\text{rxn}} \]

In each trial, the indicated solutions, initially at \(22.0\ ^\circ\text{C}\), are mixed in an insulated calorimeter of negligible heat capacity. Assume that all solutions have a density of \(1.00\text{ g/mL}\) and a specific heat capacity of \(4.18\text{ J/(g}\cdot^\circ\text{C)}\).

Trial	Volume and concentration of \(\text{HCl(aq)}\)	Volume and concentration of \(\text{NaOH(aq)}\)	Total volume
1	\(50.0\text{ mL}\) of \(1.0\text{ M}\)	\(50.0\text{ mL}\) of \(1.0\text{ M}\)	\(100.0\text{ mL}\)
2	\(50.0\text{ mL}\) of \(1.0\text{ M}\)	\(50.0\text{ mL}\) of \(2.0\text{ M}\)	\(100.0\text{ mL}\)

Which of the following correctly predicts and explains the relationship between the temperature change in Trial 2, \(\Delta T_2\), and the temperature change in Trial 1, \(\Delta T_1\)?