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Problem: Consider the following reaction:Estimate the carbon–fluorine bond energy, given that the C—C bond energy is 347 kJ/mol, the C=C bond energy is 614 kJ/mol, and the F—F bond energy is 154 kJ/mol.

🤓 Based on our data, we think this question is relevant for Professor Stec's class at UIC.

FREE Expert Solution

In calculating the enthalpy change of a reaction using bond energies, the formula is:


∆H°rxn = BE(reactants) - BE(products)


The reaction is:


In the reactant side, 

• 1 C=C single bonds will break

• 4 C-H single bonds will break

• 1 F-F single bond will also break

Bond breaking is an endothermic process. Therefore ∆H° will be positive.


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Problem Details

Consider the following reaction:

Estimate the carbon–fluorine bond energy, given that the C—C bond energy is 347 kJ/mol, the C=C bond energy is 614 kJ/mol, and the F—F bond energy is 154 kJ/mol.

Frequently Asked Questions

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. If you need more Bond Energy practice, you can also practice Bond Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Stec's class at UIC.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.