Consider the given figure and choose the correct option :

We need to determine the activation energy of the forward reaction and the relative stability of the reactants and products from the given energy profile diagram.

Diagram Analysis:

• Activation Energy of Forward Reaction ($$E_{a,\text{ fwd}}$$):
  The energy barrier from the reactant level to the peak of the transition state (activated complex) is the sum of the two vertical intervals shown:
  $$E_{a,\text{ fwd}} = E_1 + E_2$$
• Relative Stability:
  The energy level of the reactant is lower than the energy level of the product.
  Since lower energy corresponds to greater thermodynamic stability:
  $$\text{Energy of Reactant} < \text{Energy of Product} \implies \text{Reactant is more stable than Product}$$
  Thus, the product is less stable than the reactant.

Conclusion:

The activation energy for the forward reaction is $$E_1 + E_2$$, and the product is less stable than the reactant.

Answer: Option B