Use the data given below to construct a born-haber cycle to determine the heat of formation of kcl. δ h°(kj) k(s) → k(g) 89 k(g) → k (g) e- 418 cl2(g) → 2 cl(g) 244 cl(g) e- → cl-(g) -349 kcl(s) → k (g) cl-(g) 717 use the data given below to construct a born-haber cycle to determine the heat of formation of kcl. h°(kj) k(s) → k(g) 89 k(g) → k (g) e- 418 cl2(g) → 2 cl(g) 244 cl(g) e- → cl-(g) -349 kcl(s) → k (g) cl-(g) 717 158 kj -1119 kj -997 kj 631 kj -437 kj

Explanation:

The net equation will be as follows.

So, we are required to find for this reaction.

Therefore, steps involved for the above process are as follows.

Step 1:  Convert K from solid state to gaseous state

          ,     = 89 kJ

Step 2:  Ionization of gaseous K

           ,     = 418 KJ

Step 3:  Dissociation of gas into chlorine atom .

            ,   = 122 KJ

Step 4: Iozination of chlorine atom.

              ,       = -349 KJ

Step 5:  Add ion and ion formed above to get KCl .

              ,   = -717 KJ

Now, using Born-Haber cycle, value of enthalpy of the formation is calculated as follows.

                  = 89 + 418 + 122 - 349 - 717

                  = - 437 KJ/mol

Thus, we can conclude that the heat of formation of KCl is - 437 KJ/mol.

the solar system used to have much dust particles option no d