The average bond energy (enthalpy) for a c=c double bond is 614 kj/mol and that of a c−c single bond is 348 kj/mol. estimate the energy needed to break only the π bond of the double bond of 2-butene. express your answer numerically in joules per molecule.

The energy needed to break the pi bond in Joules per molecule is;

E = 4.42 × 10^(-22) J/molecule.

According to the question,

However, we must note that a double bond is made up of a pi-bond and a sigma-bond.

On the other hand, a single bond is made up of a sigma-bond.

Consequently, the energy needed to break the pi bond is given as;

However, the question requires that we express the energy in Joules per molecule.

According to Avogadro; there are 6.02 × 10²³ molecules in one mole of any substance;

Therefore, the energy needed to break the pi bond in Joules per molecule is;

E = 4.42 × 10^(-22) J/molecule.

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Bond energy or enthalpy is defined as the change in the heat content of the reaction. The energy needed to break the pi bonds in Joules per molecule is E= .

Given that,

Enthalpy for C=C bond = 614 kJ/mol

Enthalpy for C-C bond  = 348 kJ/mol

Energy required to break the pi bond will be:

E = 614 kJ/mol - 348 kJ/mol

E = 266 kJ/mol

Also, in one mole of a substance:

1 mole  = 6.022 x

The energy needed to break the pi bonds in Joules per molecule is:

Therefore, the energy needed to break the pi bond in Joules per molecule is 4.42 x J/molecule.

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increased stability in the completion of fluorine's outer shell.

6.4 cm (max) - 25 cm (min)