One method of favoring the formation of an ester is to add excess acetic acid. Suggest another method, involving the right-hand
1 answer:
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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.