Question

unit test #3
examine the figure below for the following question:
which letter represents the activation energy of the forward reaction?
a
b
c
d
none of the above

Explanation:

Activation energy is the minimum energy required for a reaction to occur. In a potential - energy diagram for a reaction, it is the energy difference between the reactants and the transition state (the highest point on the curve).

• Option A: This is the energy difference between the reactants and the products. It represents the enthalpy change ($\Delta H$) of the reaction, not the activation energy.
• Option B: This is not a standard quantity in the context of activation energy.
• Option C: This is not relevant to the activation energy concept.
• Option D: This represents the energy difference between the reactants and the transition state (the peak of the curve), which is the definition of activation energy for the forward reaction.

Answer:

D.