Consider the following reaction. H2C=CH2(g) + F2(g) ? CH2FCH2F(g) ?H = -549 kJ 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. kJ/mol

          Consider the following reaction.
H2C=CH2(g) + F2(g) ? CH2FCH2F(g) ?H = -549 kJ
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.
kJ/mol

Consider the following reaction.
H2C=CH2(g) + F2(g) ? CH2FCH2F(g) ?H = -549 kJ
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.
kJ/mol

Added by Jennifer R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Monisha Shukla

04/19/2022

Step 1

The energy required to break a bond is equal to the bond energy, so we need 614 kJ/mol to break the C=C bond and 154 kJ/mol to break the F-F bond. The energy released when a bond is formed is also equal to the bond energy. So, if we let X be the C-F bond Show more…

Show all steps

Thanks for your feedback!

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.