Question

Part C A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 13.5 kJ/mol separation of solvent 23.8 kJ/mol formation of solute-solvent interactions -89.7 kJ/mol solute Calculate the enthalpy of solution in kilojoules per mole of solute. Enter your answer numerically in kilojoules per mole of solute. View Available Hint(s) ΔHsoln Δ H s o l n Delta H_soln = nothing kJ/mol

Answer 1

To separate the solute particles i.e. to breakdown solute-solute interactions, energy is absorbed by the system

So Action enthalpy for separation of solute=13.5 kJ/mol

Similarly to breakdown solvent-solvent interactions energy is absorbed by the system

Action enthalpy for separation of solvent=23.8 kJ/mol

To form solute solvent interactions, energy is released from the system.

Action enthalpy of solute-solute interactions=-89.7 kJ/mol

Enthalpy of solution=Action enthalpy for (solute separation+ solvent separation + solute-solvent interactions)=13.5 kJ/mol+ 23.8 kJ/mol-89.7 kJ/mol=-52.4 kJ/mol