Consider the given figure and choose the correct option:
Consider the given figure and choose the correct option:
Show Hint
- Activation energy of both forward and backward reaction is \( E_1 + E_2 \) and reactant is more stable than product.
- Activation energy of backward reaction is \( E_1 \) and product is more stable than reactant.
- Activation energy of forward reaction is \( E_1 + E_2 \) and product is less stable than reactant.
- Activation energy of forward reaction is \( E_1 + E_2 \) and product is more stable than reactant.
The Correct Option is D
Approach Solution - 1
The given figure represents a typical energy profile diagram for a chemical reaction. It shows the energy of reactants, products, and the activated complex (transition state). Two energy differences are marked:
• E1: Energy difference between the product and the activated complex.
• E2: Energy difference between the reactant and the product.
1. Forward Activation Energy
The forward activation energy is the energy needed to convert reactants into the activated complex. This is the total vertical energy gap from the reactant level to the peak of the curve.
Reactant → Product = E2
Product → Activated complex = E1
So, forward activation energy = E1 + E2
2. Backward Activation Energy
Backward activation energy is the energy required for the reverse reaction (product → activated complex). This is simply the energy gap between product and the activated complex:
Backward activation energy = E1
3. Stability of Reactant vs Product
Stability is inversely related to energy: a species with lower energy is more stable.
In the diagram, the product is at a higher energy level than the reactant. Therefore, the product is less stable and the reactant is more stable.
Conclusion
• Forward activation energy = E1 + E2
• Product is less stable than reactant
These statements match exactly with Option 3.
Correct Answer: Option 3
Approach Solution -2
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