Final answer:
The heat of hydration of lithium chloride can be calculated using the lattice energy and the enthalpy of solution. In this case, the heat of hydration is 797 kJ/mol.
Step-by-step explanation:
The heat of hydration of lithium chloride can be calculated using the lattice energy and the enthalpy of solution. The heat of hydration is the energy released when one mole of ions in the gaseous phase combines with water molecules and forms hydrated ions in solution. In this case, the lattice energy of LiCl is given as 834 kJ/mol, and the enthalpy of solution is given as -37.0 kJ/mol.
To calculate the heat of hydration, we need to consider the energy required to break the ionic bonds in LiCl (lattice energy) and the energy released when the hydrated ions form in solution (enthalpy of solution).
The heat of hydration can be calculated by adding the lattice energy and the enthalpy of solution:
Heat of hydration = lattice energy + enthalpy of solution = 834 kJ/mol + (-37.0 kJ/mol) = 797 kJ/mol.