A student mixes \(50.0\text{ mL}\) of \(1.0\text{ M HCl(aq)}\) at \(22.0^\circ\text{C}\) with \(50.0\text{ mL}\) of \(1.0\text{ M NaOH(aq)}\) at \(22.0^\circ\text{C}\) in an insulated coffee-cup calorimeter. The temperature of the mixture increases to a maximum of \(28.5^\circ\text{C}\), corresponding to a \(\Delta T\) of \(6.5^\circ\text{C}\).

The student repeats the experiment using \(100.0\text{ mL}\) of \(1.0\text{ M HCl(aq)}\) and \(100.0\text{ mL}\) of \(1.0\text{ M NaOH(aq)}\), both initially at \(22.0^\circ\text{C}\). Assuming the densities and specific heat capacities of all solutions are equal to those of water and heat loss to the surroundings is negligible, which of the following best predicts and explains the expected temperature change, \(\Delta T\), for the second trial?