Dissociation enthalpies of methane and Ethane are 400 , 680kilo calorie per mole respectively. TheC-C Bond energy in ethane is?

Question

Answer

Explanation of C-C Bond Energy in Ethane

Dissociation Enthalpies of Methane and Ethane

The dissociation enthalpy of methane is 400 kilo calorie per mole.

The dissociation enthalpy of ethane is 680 kilo calorie per mole.

Definition of Dissociation Enthalpy

Dissociation enthalpy is the amount of energy required to break a bond in a molecule, resulting in the formation of two separate atoms or molecules.

C-C Bond Energy in Ethane

The C-C bond energy in ethane can be calculated by subtracting the dissociation enthalpy of methane from the dissociation enthalpy of ethane.

C-C bond energy = dissociation enthalpy of ethane - dissociation enthalpy of methane

Therefore, C-C bond energy in ethane = 680 - 400 = 280 kilo calorie per mole.

Explanation of C-C Bond Energy in Ethane

The C-C bond energy in ethane is stronger than the C-H bond energy in methane. This is because the C-C bond is a covalent bond between two carbon atoms, which have a higher electronegativity than hydrogen. This results in a stronger bond, as the electrons are shared more equally between the two carbon atoms.

In addition, the C-C bond in ethane is a sigma bond, which is stronger than the pi bond in a double bond. This is because the sigma bond is formed by the overlap of two atomic orbitals along the axis connecting the two atoms, while the pi bond is formed by the sideways overlap of two atomic orbitals.

Overall, the C-C bond energy in ethane is higher than the C-H bond energy in methane due to the stronger covalent bond between two carbon atoms and the type of bond formed.

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