Statment 1`|Delta_(f)H|" of "(H_(2)O,l)gt|Delta_(f)H|" of "(H_(2)O,g)`
Statment 2 `DeltaH_("condensation")` is negative.
(a)If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
(b)If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
(c)If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
(d)If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To analyze the statements given in the question, we need to understand the concepts of enthalpy of formation and condensation in the context of water in its liquid and gaseous states.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- Statement 1 claims that the enthalpy of formation of water in the liquid state (ΔH_f(H₂O, l)) is greater than the enthalpy of formation of water in the gaseous state (ΔH_f(H₂O, g)).
- This statement is **FALSE**. The enthalpy of formation of a substance in the gaseous state is generally higher than that of the liquid state because energy is required to convert the liquid into gas (vaporization). Therefore, ΔH_f(H₂O, l) < ΔH_f(H₂O, g).

2. **Understanding Statement 2**:
- Statement 2 states that the enthalpy change of condensation (ΔH_condensation) is negative.
- This statement is **TRUE**. When a gas condenses into a liquid, it releases energy, which means that the enthalpy change for condensation is negative.

3. **Evaluating the Statements**:
- Since Statement 1 is FALSE and Statement 2 is TRUE, we can conclude that the correct option is (d): If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE.

### Final Answer:
The correct option is (d): If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE.