Lithium iodide has a lattice energy of -7.3x10^2kj.mol and heat of hydration of -793kj.mol. Find the heat of solution for lithium iodide.
H solution= H solute + H hydration
H solute = -H lattice
H solution = -(-7.3x10^2) kj/mol + (-793) kj/mol
H solution = -63 kj/mol
The heat of solution can be calculated using the equation:
Heat of solution = Lattice energy + Heat of hydration
Given:
Lattice energy = -7.3 x 10^2 kJ/mol
Heat of hydration = -793 kJ/mol
Substituting the values into the equation:
Heat of solution = -7.3 x 10^2 kJ/mol + (-793 kJ/mol)
Calculating the sum:
Heat of solution = -7.3 x 10^2 kJ/mol - 793 kJ/mol
Heat of solution = -730 kJ/mol - 793 kJ/mol
Heat of solution = -1523 kJ/mol
Therefore, the heat of solution for lithium iodide is -1523 kJ/mol.
To find the heat of solution for lithium iodide, we need to use the concept of lattice energy and heat of hydration.
The heat of solution is the overall energy change when a solute dissolves in a solvent. It takes into account both the energy required to break the solute-solute interactions (lattice energy) and the energy released or absorbed when the solute interacts with the solvent (hydration energy).
The heat of solution can be calculated using the following equation:
Heat of solution = lattice energy + heat of hydration
Given:
Lattice energy of lithium iodide (LiI) = -7.3x10^2 kJ/mol (negative sign indicates energy released during lattice formation)
Heat of hydration of lithium iodide (LiI) = -793 kJ/mol (negative sign indicates energy released during hydration)
To find the heat of solution for lithium iodide, we simply add the lattice energy and heat of hydration values:
Heat of solution = (-7.3x10^2 kJ/mol) + (-793 kJ/mol)
Heat of solution = -7.3x10^2 kJ/mol - 793 kJ/mol
Heat of solution = -2.159x10^3 kJ/mol
Therefore, the heat of solution for lithium iodide is -2.159x10^3 kJ/mol. The negative sign indicates that the dissolution of lithium iodide is an exothermic process, meaning it releases energy.