Lithium iodide has a lattice energy of -7.3 x 102(kj/mol) and a heat of hydration of -793 kj/mol. find the heat of solution for lithium iodide and determine how much heat is evolved or absorbed when 15.0 g of lithium iodide completely dissolves in water.

Given molecule Lithium iodide (LiI)

Heat of hydration = -793 kj/mol

Lattice energy = -730 kJ/mol

Heat of hydration = Heat of solution - Lattice energy

Heat of solution = Hydration + Lattice = -793 + (- 730) = -1523 kJ/mol

Now,

Mass of LiI = 15.0 g

molar mass of LiI = 134 g/mol

# moles of LiI = 15/134 = 0.112 moles

Heat of solution for 1 mole of LiI = -1523 KJ

Therefore, for 0.112 moles of LiI the corresponding heat is

= 0.112 *(-1532) = 171.6 kJ

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

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