Concept:Activation energy (\( E_a \)) is the energy difference between the reactants and the transition state (activated complex).
Solution:- In an endothermic reaction, the products have a higher potential energy than the reactants, and a large amount of energy must be absorbed to break the strong initial bonds.
- Because the reactants sit at a much lower energy well relative to the transition state, the "energy hill" they must climb is significantly steeper.
- Therefore, endothermic reactions typically require a greater activation energy (\( E_a \)) compared to exothermic reactions, where the reactants are inherently closer to the transition state energy.
Why other options are incorrect:If it required smaller or equal \( E_a \), it would likely not be heavily endothermic. All standard reactions require
some \( E_a \).
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