Assertion : In a metabolic reaction with a negative `DeltaG`, the products contain less free energy than the reactants, energy is released and entropy increases.
Such negative `DeltaG` reaction is spontaneous because it occurs without an input of energy .

Options

A. If both the assertion and reason are true statement and reason is correct explanation of the assertion .
B. If both the assertion and reason are true statement but reason is not a correct explanation of the assertion .
C. If the assertion is true but the reason is a false statement.
D. If both assertion and reason are false statements.

Answer

To solve the question regarding the assertion and reason about metabolic reactions and Gibbs free energy (ΔG), we can break it down step by step.

### Step-by-Step Solution:

1. **Understanding Gibbs Free Energy (ΔG)**:
- Gibbs free energy (ΔG) is a thermodynamic quantity that represents the maximum reversible work that can be performed by a thermodynamic system at constant temperature and pressure.
- The formula for ΔG is given by:
\[ ΔG = ΔH - TΔS \]
- Here, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.

2. **Analyzing the Assertion**:
- The assertion states that in a metabolic reaction with a negative ΔG, the products contain less free energy than the reactants, energy is released, and entropy increases.
- This is true because a negative ΔG indicates that the reaction is exergonic (releases energy) and that the products are at a lower energy state compared to the reactants.

3. **Understanding Entropy**:
- Entropy (ΔS) is a measure of disorder or randomness in a system. In spontaneous reactions, the entropy of the universe tends to increase.
- Therefore, in reactions with negative ΔG, it is typical for the entropy of the system to increase, aligning with the assertion.

4. **Analyzing the Reason**:
- The reason states that such negative ΔG reactions are spontaneous because they occur without an input of energy.
- This is also true. A spontaneous reaction is one that can occur without an external energy source, which is consistent with the characteristics of reactions that have a negative ΔG.

5. **Conclusion**:
- Both the assertion and the reason are true statements. Moreover, the reason correctly explains the assertion.
- Therefore, the correct option is that both the assertion and reason are true, and the reason is the correct explanation of the assertion.

### Final Answer:
The correct option is **Option A**: Both assertion and reason are true statements, and the reason is the correct explanation of the assertion.

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