Assertion : The boiling points of given compounds follow the order :
`CH_(3)CH_(2)CH_(2)CHO ~~CH_(3)CH_(2)CH_(2)CH_(2)CH_(3) lt CH_(3)CH_(2)CH_(2)CH_(2)OH ~~ H_(5)C_(2)OC_(2)H_(5)`
Reason : Boiling point depends upon molecualr mass only.

Options

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

Explanation

To solve the question regarding the boiling points of the given compounds and the assertion and reason provided, we will analyze the compounds and their boiling points step by step.

### Step 1: Identify the Compounds
The compounds mentioned in the assertion are:
1. **CH₃CH₂CH₂CHO** (Butanal)
2. **CH₃CH₂CH₂CH₂CH₃** (Pentane)
3. **CH₃CH₂CH₂CH₂OH** (Butanol)
4. **H₅C₂OC₂H₅** (Diethyl ether)

### Step 2: Understand Boiling Point Influences
Boiling points are influenced by several factors, including:
- Molecular mass
- Intermolecular forces (hydrogen bonding, dipole-dipole interactions, Van der Waals forces)

### Step 3: Analyze Each Compound
- **Butanal (CH₃CH₂CH₂CHO)**: This compound has a carbonyl group (C=O) which allows for dipole-dipole interactions.
- **Pentane (CH₃CH₂CH₂CH₂CH₃)**: This is a non-polar hydrocarbon with only Van der Waals forces, leading to a lower boiling point.
- **Butanol (CH₃CH₂CH₂CH₂OH)**: The presence of an -OH group allows for hydrogen bonding, which significantly increases the boiling point.
- **Diethyl ether (H₅C₂OC₂H₅)**: This compound has an ether functional group, which allows for some dipole interactions but is not as strong as hydrogen bonding.

### Step 4: Compare Boiling Points
Based on the types of intermolecular forces:
- **Butanol** has the highest boiling point due to extensive hydrogen bonding.
- **Butanal** has a higher boiling point than pentane due to dipole-dipole interactions.
- **Pentane** has the lowest boiling point due to only having Van der Waals forces.
- **Diethyl ether** has a boiling point that is generally lower than butanol but higher than pentane due to dipole interactions.

### Step 5: Order of Boiling Points
The correct order of boiling points based on the analysis should be:
1. **Butanol (CH₃CH₂CH₂CH₂OH)** >
2. **Butanal (CH₃CH₂CH₂CHO)** >
3. **Diethyl ether (H₅C₂OC₂H₅)** >
4. **Pentane (CH₃CH₂CH₂CH₂CH₃)**

### Conclusion
- **Assertion**: The order of boiling points as stated is incorrect.
- **Reason**: The reason provided is also incorrect since boiling points depend not only on molecular mass but also on the nature of intermolecular forces.

### Final Answer
Both the assertion and reason are false.