Respuesta :
The energy needed to break the pi bond in Joules per molecule is;
E = 4.42 × 10^(-22) J/molecule.
According to the question,
- The average bond energy (enthalpy) for a C=C double bond is 614 kJ/mol
- That of a C−C single bond is 348 kJ/mol.
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;
- E = 614 kJ/mol - 348 kJ/mol
- E = 266 kJ/mol
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 = 266/6.02 × 10²³
E = 4.42 × 10^(-22) J/molecule.
Read more:
https://brainly.com/question/18873664
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= [tex]4.42 \times 10^{-22} \text{J/molecule}[/tex].
Given that,
Enthalpy for C=C bond = 614 kJ/mol
Enthalpy for C-C bond = 348 kJ/mol
- Sigma bonds are the single bonds, which are formed by the head to head overlapping of orbitals.
- Pi bonds are double or triple bonds that are formed by the perpendicular overlapping of orbitals along the axis of single bonds.
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 [tex]10^{23}[/tex]
The energy needed to break the pi bonds in Joules per molecule is:
[tex]\text {E}&=\dfrac{266}{6.022 \times 10^{23}}\\\\\text {E}&=4.42\times 10^{23}} \text{J/molecule}[/tex]
Therefore, the energy needed to break the pi bond in Joules per molecule is 4.42 x [tex]10^{-22}[/tex] J/molecule.
To know more about bond energy, refer to the following link:
https://brainly.com/question/14299954?referrer=searchResults
