What is the sign of ΔHsoln, and how will the temperature change when a solute dissolves with the following enthalpy changes? ΔH_solute = +56 kJ/mol, ΔH_solvent = +34 kJ/mol, ΔH_{solute-solvent} = -125 kJ/mol.

Verified step by step guidance

1. Step 1: Understand the concept of enthalpy of solution (ΔH_{soln}). It is the overall energy change when a solute dissolves in a solvent, and it can be calculated using the formula: ΔH_{soln} = ΔH_{solute} + ΔH_{solvent} + ΔH_{solute-solvent}.
2. Step 2: Identify the given enthalpy changes: ΔH_{solute} = +56 kJ/mol, ΔH_{solvent} = +34 kJ/mol, and ΔH_{solute-solvent} = -125 kJ/mol.
3. Step 3: Substitute the given values into the formula for ΔH_{soln}: ΔH_{soln} = (+56 kJ/mol) + (+34 kJ/mol) + (-125 kJ/mol).
4. Step 4: Analyze the sign of ΔH_{soln}. If the result is negative, the process is exothermic, meaning the solution releases heat and the temperature increases. If positive, the process is endothermic, meaning the solution absorbs heat and the temperature decreases.
5. Step 5: Calculate the sum of the enthalpy changes to determine the sign of ΔH_{soln} and predict the temperature change accordingly.