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The energies of activation for forward and reverse reactions for $A_{2} + B_{2} \Leftrightarrow 2 A B$ are 180 kJ/mol and 200 kJ/mol, respectively. The presence of a catalyst lowers the activation energy of both forward and reverse) reactions by 100 kJ/mol. The enthalpy change of the reaction $A_{2} + B_{2} \to 2 A B$ in the presence of a catalyst will be (in kJ/mol)

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120

-20

300

+20

answer is A.

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Detailed Solution

$Δ H = 200 - 180 k J = 20 k J$

Forward reaction is exothermic, so $Δ H = - 20 k J$ . Catalyst does not alter $Δ H$

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