Each question contains STATEMENT-I(Assertion) and STATEMENT-2(Reason).the statement carefully and mark the correct answer according to the instruction given below:
STATEMENT - 1 : The boiling point of 0.1 M urea solution is less than that of 0.1 M KClsolution.
STATEMENT - 2 : Elevation of boiling point is directly proportional to the number of moles of non-volatile solute particles present in the solution.

Options

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

Answer

To solve the question regarding the boiling point of urea and KCl solutions, let's break it down step by step:

### Step 1: Understand the Statements
- **Statement 1**: The boiling point of 0.1 M urea solution is less than that of 0.1 M KCl solution.
- **Statement 2**: Elevation of boiling point is directly proportional to the number of moles of non-volatile solute particles present in the solution.

### Step 2: Analyze Statement 1
To determine the validity of Statement 1, we need to consider the concept of boiling point elevation, which is a colligative property. Colligative properties depend on the number of solute particles in a solution, not on their identity.

### Step 3: Understand the van 't Hoff Factor (i)
The van 't Hoff factor (i) indicates the number of particles into which a solute dissociates in solution:
- For urea (a non-electrolyte), \( i = 1 \) (it does not dissociate).
- For KCl (an electrolyte), \( i = 2 \) (it dissociates into K\(^+\) and Cl\(^-\)).

### Step 4: Apply the Formula for Boiling Point Elevation
The elevation in boiling point (\( \Delta T_b \)) can be calculated using the formula:
\[ \Delta T_b = i \cdot K_b \cdot m \]
Where:
- \( K_b \) is the ebullioscopic constant (a property of the solvent),
- \( m \) is the molality of the solution.

Since both solutions have the same molarity (0.1 M), we can focus on the van 't Hoff factor (i):
- For urea: \( \Delta T_b = 1 \cdot K_b \cdot 0.1 \)
- For KCl: \( \Delta T_b = 2 \cdot K_b \cdot 0.1 \)

### Step 5: Compare the Elevation of Boiling Points
Since \( i \) for KCl is greater than that for urea, the boiling point elevation for KCl will be greater than that for urea. Therefore, the boiling point of the KCl solution will be higher than that of the urea solution. This confirms that:
- **Statement 1** is true: The boiling point of 0.1 M urea solution is indeed less than that of 0.1 M KCl solution.

### Step 6: Analyze Statement 2
Statement 2 states that the elevation of boiling point is directly proportional to the number of moles of non-volatile solute particles present in the solution. This is true because colligative properties depend on the number of solute particles.

### Step 7: Conclusion
Both statements are correct, and Statement 2 provides the correct explanation for Statement 1. Therefore, the final answer is:
- Both statements are true, and Statement 2 is the correct explanation of Statement 1.