Ammonia is more easy to liquefy than oxygen, then which of the following is true about oxygen as the reason for this fact?

Options

A. It has high critical temperature.
B. It has low critical temperature
C. It has high bond dissociation
D. Its electronegatively is high

Answer

To solve the question regarding why ammonia (NH3) is easier to liquefy than oxygen (O2), we can analyze the properties of both substances, particularly focusing on their intermolecular forces and critical temperatures.

### Step-by-Step Solution:

1. **Understanding Liquefaction**: Liquefaction refers to the process of converting a gas into a liquid. The ease of liquefaction is influenced by the strength of intermolecular forces and the critical temperature of the substance.

2. **Intermolecular Forces**: Ammonia (NH3) exhibits stronger intermolecular forces compared to oxygen (O2). This is primarily due to hydrogen bonding in ammonia, which is a significant factor that increases the attractive forces between its molecules.

3. **Van der Waals Forces**: The Van der Waals forces in ammonia are stronger than those in oxygen. This is indicated by a higher Van der Waals constant (A) for ammonia, which signifies stronger intermolecular attractions.

4. **Critical Temperature**: The critical temperature (Tc) is the temperature above which a substance cannot exist as a liquid, regardless of the pressure applied. Ammonia has a higher critical temperature compared to oxygen, meaning it can be liquefied at higher temperatures.

5. **Conclusion**: Because ammonia has stronger intermolecular forces (due to hydrogen bonding) and a higher critical temperature, it is easier to liquefy than oxygen, which has weaker Van der Waals forces and a lower critical temperature.

### Final Statement:
Thus, the true statement regarding oxygen as the reason for ammonia being easier to liquefy is that oxygen has a low critical temperature and weaker intermolecular forces compared to ammonia.

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