Based on the following data,what is the Cl-Cl bond energy? H₂(g)+ Cl₂(g)$\to$ HCl(g); $\Delta$_rH $\circ$ = -92.31 kJ/mol-rxn

Question

Quizplus · Accepted Answer

In the given reaction, we need to break one Cl-Cl bond and form one H-Cl bond. 
Bond energy of H-Cl is 428 kJ/mol. 
To calculate the bond energy of Cl-Cl, let's first find the enthalpy change of the reaction:

ΔH = -92.31 kJ/mol-rxn

Now, let's calculate the enthalpy change for the breaking of one Cl-Cl bond and forming one H-Cl bond:

ΔH = Energy required to break Cl-Cl bond - Energy released in forming H-Cl bond 
ΔH = (Cl-Cl bond energy) - 428 kJ/mol

We can solve for Cl-Cl bond energy:

Cl-Cl bond energy = ΔH + 428 kJ/mol

Cl-Cl bond energy = -92.31 kJ/mol + 428 kJ/mol = 335.69 kJ/mol

Therefore, the Cl-Cl bond energy is 335.69 kJ/mol, which corresponds to choice (B) as the correct answer.

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