Respuesta :
Explanation:
The net equation will be as follows.
[tex]K(s) + Cl_{2}(g) \rightarrow KCl(s)[/tex]
So, we are required to find [tex]\Delta H_{formation}[/tex] for this reaction.
Therefore, steps involved for the above process are as follows.
Step 1: Convert K from solid state to gaseous state
[tex]K(s) \rightarrow K(g)[/tex], [tex]\Delta H_{1}[/tex] = 89 kJ
Step 2: Ionization of gaseous K
[tex]K(g) \rightarrow K^{+}(g) + e^{-}[/tex], [tex]H_{2}[/tex] = 418 KJ
Step 3: Dissociation of [tex]Cl_{2}[/tex] gas into chlorine atom .
[tex]\frac{1}{2} Cl_{2}(g) \rightarrow Cl(g)[/tex], [tex]\Delta H_{3} = \frac{244}{2}[/tex] = 122 KJ
Step 4: Iozination of chlorine atom.
[tex]Cl(g) + e^{-} \rightarro Cl^{-}(g)[/tex], [tex]H_{4}[/tex] = -349 KJ
Step 5: Add [tex]K^{+}[/tex] ion and [tex]Cl^{-}[/tex] ion formed above to get KCl .
[tex]K^{+}(g) + Cl^{-}(g) \rightarrow KCl(s)[/tex], [tex]H_{5}[/tex] = -717 KJ
Now, using Born-Haber cycle, value of enthalpy of the formation is calculated as follows.
[tex]\Delta H_{f} = \DeltaH_{1} + \Delta H_{2} + \Delta H_{3} + \Delta H_{4} + \Delta H_{5}[/tex]
= 89 + 418 + 122 - 349 - 717
= - 437 KJ/mol
Thus, we can conclude that the heat of formation of KCl is - 437 KJ/mol.
Answer:
The net energy of the reaction calculated by the Born-Haber cycle is -437 kJ/mole.
Explanation:
Born-Haber cycles have been used to determine the energies of the reaction. In a cycle, the net energy of the reaction can be calculated.
The given reaction is the formation of KCl.
[tex]\rm K\;(s)\;+\;Cl_2\;(g)\;\rightarrow\;KCl\;(s)[/tex]
For the reaction to proceed, K is to be converted to the gaseous state.
The energy is 89 K.
The K has to be in the ionic form for reaction. The energy for an ionic form of K is 418 K.
The [tex]\rm Cl_2[/tex] has to be converted to the atomic form and further to the ionic form. For this, the energies for conversion to Cl atom, and to Cl ion are: 122 kJ and -349 kJ respectively.
The energy required for the formation of KCL molecules is -717 kJ.
The net energy or Born-Haber cycle for the reaction will be the sum of all the energies.
[tex]\Delta[/tex]H = 89 + 418 + (-349 + (-717) kJ
[tex]\Delta[/tex]H = -437 kJ/mole.
The net energy for the reaction will be -437 kJ/mole.
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