Problem: How does the bond energy of HCl(g) differ from the standard enthalpy of formation of HCl(g)?

FREE Expert Solution

The bond energy determines the strength of the bond in a compound.

▪ the higher the bond energy, the higher is the energy required to break up the molecule/compound into its individual atoms


The standard enthalpy of formation is the change in enthalpy when one mole of a substance in the standard state is formed from its pure elements (formation of covalent bond) 

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How does the bond energy of HCl(g) differ from the standard enthalpy of formation of HCl(g)?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. You can view video lessons to learn Bond Energy. Or if you need more Bond Energy practice, you can also practice Bond Energy practice problems.

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Based on our data, we think this problem is relevant for Professor Hauck Jr's class at UNO.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.