Question

Could someone explain how to solve this for me?

We have been studying fluoride in drinking water. If you were to examine your toothpaste one of the active ingredient is most likely to be sodium fluoride. Given theinformation below write the equation associated with each one of the following energies,daw the Born Haber Cycle and calculate the lattice energy for the formation of Sodiumfluoride.

First Ionization energy of Na: 496 kJ/molFirst

Electron affinity of F: –328 kJ/mol

Enthalpy of atomization Na: 108 kJ/molF2

bond energy: 159 kJ/mol

Enthalpy of formation of NaF(s) = –574 kJ/mol

Answer 1

Given data

First Ionization energy of Na: 496 kJ/mol                    Na(g) ------->Na⁺ + e^-

Electron affinity of F: –328 kJ/mol                               F(g) + e^- -------------> 2F(g)

Enthalpy of atomization Na: 108 kJ/mol Na(s) -------------> Na(g)

bond energy of fluorine gas: 159 kJ/mol                    F₂(g)------------------> 2F(g)

Enthalpy of formation of NaF(s) = –574 kJ/mol          Na(s) + 1/2F₂ ---------> NaF

Using Born Haber cycle

Enthalpy of formation of NaF_(s) = Enthalpy of atomization Na + First Ionization energy of Na + bond energy of fluorine gas + Electron affinity of F + Lattice energy of NaF

-574 = 108 + 496 + 159 -328 + Lattice energy      (all the energies are in kj/mol)

Lattice energy = -574 -108-496-159+328 = -1009 kj/mol