Question

6) There is Something called the lattice Energy.Is that the energy needed to break the ionic bound between, in this case Mg2+...O ? in a mgso4 dissolved in distilled water?
7) How do I calculate how much energy i need to break all the Mg2+....O bounds in a 100 ml solution of Mgso4, at 20 degrees.
8) Would the calculation in 7) be different if i used mgso4*7h20 or mgso4*6h20 in the saturated solution.

Answer 1

Answer on Question #71167 – Chemistry – General Chemistry

6) There is something called the lattice energy. Is that the energy needed to break the ionic bound between, in this case Mg²⁺...O? in a MgSO₄ dissolved in distilled water?

7) How do I calculate how much energy I need to break all the Mg²⁺...O bounds in a 100 ml solution of MgSO₄ at 20 degrees.

8) Would the calculation in 7) be different if I used MgSO₄·7H₂O or MgSO₄·6H₂O in the saturated solution.

Solution:

Lattice energy is the energy required to break apart an ionic solid and convert its component atoms into gaseous ions, in this case Mg²⁺...SO₄²⁻.

You can use a Hess's Law cycle (in this case called a Born-Haber cycle) involving enthalpy changes which can be measured.

Enthalpy of lattice formation (lattice energy) of MgSO₄ = -2833 kJ·mol⁻¹

Will be no differ if you use MgSO₄·7H₂O or MgSO₄·6H₂O, because crystallized water dissolve in solution. For calculations of the lattice energy you need only MgSO₄

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