🤓 Based on our data, we think this question is relevant for Professor All Professors' class at TAMU.
First, we look at the expansion of the solvent and solute. The enthalpy change (ΔH1 and ΔH2) must be greater than zero because they need to absorb energy (endothermic) in order to overcome the intermolecular forces that bind those compounds together.
Also, it is important to note that the solute went from a more ordered/tightly packed structure than the solvent. This means that it would require more energy to change it to the expanded form.
So the relative magnitudes and charges are:
For the following solute–solvent combinations, state the sign and relative magnitudes for ΔH1, ΔH2, ΔH3, and ΔHsoln (as defined in Fig. 10‑1 of the text). Explain your answers.