Difference between Enthalpy of Atomization and bond Enthalpy with specific example .. .. ((((Please don't copy your answer from google cause I didn't find there helpful if you know then only answer)))
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Enthalpy of atomization is the amount of enthalpy change when a compound's bonds are broken and the component atoms are reduced to individual atoms.
The enthalpy of bond dissociation is the energy needed to break a single bond (such as C-H in a methane molecule) .
So in methane there are 4 C-H bonds and so the bond dissociation enthalpy of a C-H bond would be around 0.25 times the atomisation enthalpy of methane.
Combustion enthalpy is not equal to formation enthalpy.
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Types of Enthalpy: Atomisation
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Explanation:
Find the side of a square whose perimeter is 24 m.