Statement-1 : All the exothermic reactions are spontaneous.
And
Statement-2 : For a spontaneous reaction, `Delta`G must be negative.

Options

A. Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True, Statement-2 is True, Statement-2 is Not a correct explanation for Statement-1
C. Statement-1 is True, Statement-2 is False
D. Statement-1 is False, Statement-2 is True

Answer

To analyze the statements provided in the question, we will evaluate each statement based on thermodynamic principles.

### Step-by-Step Solution:

1. **Understanding Statement-1**:
- The statement claims that "All the exothermic reactions are spontaneous."
- Exothermic reactions are those that release heat (ΔH < 0). However, not all exothermic reactions are spontaneous. Spontaneity also depends on the change in entropy (ΔS) and temperature (T). Therefore, this statement is **false**.

2. **Understanding Statement-2**:
- The statement claims that "For a spontaneous reaction, ΔG must be negative."
- This is a fundamental principle in thermodynamics. The Gibbs free energy change (ΔG) indicates the spontaneity of a reaction. If ΔG < 0, the reaction is spontaneous. Therefore, this statement is **true**.

3. **Conclusion**:
- Since Statement-1 is false and Statement-2 is true, we can conclude that the correct option is that Statement-1 is false and Statement-2 is true.

### Final Answer:
The correct option is: **Statement-1 is false, Statement-2 is true.**

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