Use average bond energies to calculate δhrxn for the following hydrogenation reaction: h2c=ch2(g)+h2(g)→h3c−ch3(g)

Using average bond energies, the enthalpy of reaction for the hydrogenation of ethane is 2945.4 kJ/mol.

Let's consider the following hydrogenation reaction.

H₂C=CH₂(g) + H₂(g) → H₃C−CH₃(g)

Given the average bond energies (ΔH(bond)) we can calculate the enthalpy of the reaction (ΔHrxn) using the following equation.

The bonds broken, with their respective bond energies are:

H₂C=CH₂

H₂

The bonds formed, with their respective bond energies are:

H₃C−CH₃

The enthalpy of the reaction is:

Using average bond energies, the enthalpy of reaction for the hydrogenation of ethane is 2945.4 kJ/mol.

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The enthalpy of the hydrogenation reaction of ethane is 2945.4 kJ/mol.

The reaction is,

The bond energies of reactant and products are,

C=C (615.0 kJ/mol)

C-C (347.3 kJ/mol)

C-H (416.2 kJ/mol)

H-H (435.1 kJ/mol)

put this value in The Enthalpy formula,

So, we can conclude that the enthalpy of the given hydrogenation reaction of ethane is 2945.4 kJ/mol.

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