In the formation of the ionic bond which gives stability to the potassium chlori

Question

In the formation of the ionic bond which gives stability to the potassium chloride are involved energy steps which can be represented by Born-Haber cycle. The KCl forming reaction (s) and steps are mentioned below:(Make step by step)

Step I: Converting K (s) K (g); ?Hentalpia sublimation = + 90 kJ / mol
Step II: Dissociation ½ mole of Cl2 (g) in isolated atoms Cl (g); ?Hentalpia dedissociação = +121 kJ / mol
Step III: Ionization one mole of K atoms (g); ?Henergia ionization + = 419 kJ / mol
Step IV: Addition of 1 mol to 1 mol of electrons in single atoms of Cl (g); Electronic ?Hafirnidade = - 349 kJ / mol.
Step V: Combination 1 mol of K + ions (g) with 1 mole of chloride ions Cl- (g); DH = - 717 kJ / mol.
With respect to information and the above-mentioned data, it is correct to say that the standard enthalpy
formation of potassium chloride in kJ / mol is:

Explanation / Answer

Formation of KCl by Born-Haber cycle,

dHof = 90 + 121 + 419 - 349 - 717 = -436 kJ/mol

the standard enthalpy of formation of KCl is,

B) -436 kJ/mol

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