During spontaneous ischage of an electrochemical cell Gibb's free energy will

Options

A. Increase
B. Decrease
C. Not change
D. Be infinity

Answer

To solve the question regarding the behavior of Gibbs free energy during the spontaneous discharge of an electrochemical cell, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Spontaneous Reactions**:
- A spontaneous reaction in an electrochemical cell occurs without external intervention. This is characterized by a negative change in Gibbs free energy (ΔG).

2. **Relationship Between Gibbs Free Energy and Cell Potential**:
- The relationship between Gibbs free energy change (ΔG) and the standard cell potential (E°cell) is given by the equation:
\[ \Delta G = -nFE_{cell}^o \]
where:
- \( n \) = number of moles of electrons transferred in the reaction,
- \( F \) = Faraday's constant (approximately 96485 C/mol),
- \( E_{cell}^o \) = standard cell potential.

3. **Sign of ΔG and E°cell**:
- For a spontaneous reaction:
- ΔG < 0 (negative)
- E°cell > 0 (positive)
- This indicates that the Gibbs free energy decreases while the cell potential increases.

4. **Conclusion**:
- Therefore, during the spontaneous discharge of an electrochemical cell, Gibbs free energy (ΔG) will decrease, indicating that it becomes more negative.

### Final Answer:
During the spontaneous discharge of an electrochemical cell, Gibbs free energy will decrease (ΔG < 0).

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