For endothermic reaction:
Correct answer: C. Forward activation energy > reverse activation energy
- A. Forward activation energy < reverse activation energy
- B. Forward activation energy = reverse activation energy
- C. Forward activation energy > reverse activation energy
- D. No change
Explanation
In an endothermic reaction, the forward reaction generally requires more energy than the reverse reaction. This means that more energy is needed to initiate and sustain the forward reaction compared to the reverse reaction. It's like the forward reaction absorbs heat or energy from the surroundings, making it endothermic.
This question appeared on the KMU Centralized Admission Test 2020 paper, which you can sit online with every answer explained.
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About Activation Energy and Activated Complex
Activation energy is the minimum energy reactant particles need to form the activated complex, or transition state, during a reaction. Energy profile diagrams show the forward and reverse activation energies, while catalysts provide an alternative pathway with lower activation energy without changing the reaction enthalpy.
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