Determination of lattice energy of K C l using Born-Haber cycle has to be explained. The law for the basis of this method has to be outlined. Concept Introduction: Born-Haber cycle is based on Hess’s law to calculate the lattice enthalpy of ionic compounds and deals with energy changes in formation of ionic compounds. The energy released when gaseous state ions of unlike charges that are infinitely farther apart combine to form a stable ionic solid is called Lattice energy . Conversely, the energy required to break the electrostatic force of attraction between the ions of unlike charges in the ionic solid and revert them to gaseous state is also termed as Lattice energy of an ionic solid. Hess’s law is applied to calculate the enthalpy changes in a reaction. According to Hess’s law – “The overall enthalpy change of a reaction is equal to the sum of the enthalpy changes involving in each and every individual steps in the reaction.” Thus if a reaction involves ‘n’ steps then enthalpy change Δ H ° of the reaction is, Δ H ° = Δ H 1 ° + Δ H 2 ° + Δ H 3 ° .... + Δ H n °

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Chapter 9, Problem 9.22QP

Interpretation Introduction

Interpretation:

Determination of lattice energy of KCl using Born-Haber cycle has to be explained. The law for the basis of this method has to be outlined.

Concept Introduction:

Born-Haber cycle is based on Hess’s law to calculate the lattice enthalpy of ionic compounds and deals with energy changes in formation of ionic compounds.

The energy released when gaseous state ions of unlike charges that are infinitely farther apart combine to form a stable ionic solid is called Lattice energy. Conversely, the energy required to break the electrostatic force of attraction between the ions of unlike charges in the ionic solid and revert them to gaseous state is also termed as Lattice energy of an ionic solid.

Hess’s law is applied to calculate the enthalpy changes in a reaction. According to Hess’s law – “The overall enthalpy change of a reaction is equal to the sum of the enthalpy changes involving in each and every individual steps in the reaction.” Thus if a reaction involves ‘n’ steps then enthalpy change ΔH° of the reaction is,

ΔH°= ΔH1°+ΔH2°+ΔH3°....+ΔHn°

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