Question

The enthalpy of solution for LiCl is -37.00 kJ/mol. What can you conclude about the relative magnitudes of the absolute values of ΔHsolute and ΔHhydration, where ΔHsolute is the heat associated with separating the solute particles and ΔHhydration is the heat associated with dissolving the solute particles in water?

-ΔHsolute| < |ΔHhydration|
-|ΔHsolute| > |ΔHhydration|
-|ΔHsolute| = |ΔHhydration|
-none of the above (nothing can be concluded about the relative magnitudes)

Answer 1

Based on the given information, we can conclude that |-ΔHsolute| > |ΔHhydration|. The enthalpy of solution, which is -37.00 kJ/mol in this case, represents the heat released when the solute particles are dissolved in water. ΔHhydration must be greater in magnitude than |-ΔHsolute| in order for the dissolution process to be exothermic.

Step-by-step explanation:

Based on the given information, we can conclude that |-ΔHsolute| > |ΔHhydration|.

The enthalpy of solution, which is -37.00 kJ/mol in this case, represents the heat released when the solute particles are dissolved in water. Since this value is negative, it indicates an exothermic process where heat is being released.

On the other hand, ΔHhydration represents the heat absorbed when the solute particles are surrounded by water molecules. This value is not given in the question, but based on the given options, we can infer that it must be greater in magnitude than |-ΔHsolute| because ΔHhydration is typically positive in order for the dissolution process to be exothermic. Therefore, |ΔHhydration| > |-ΔHsolute|.