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NH(3) can be liquefied at ordinary tempe...

`NH_(3)` can be liquefied at ordinary temperature without the application of pressure. But `O_(2)` cannot be because :

A

its critical temperature is very high

B

its critical temperature is very low

C

its critical temperature is modrate

D

its critical temperature is higher than that of ammonia.

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To understand why `NH3` (ammonia) can be liquefied at ordinary temperatures without the application of pressure, while `O2` (oxygen) cannot, we need to consider the concept of critical temperature. ### Step-by-Step Solution: 1. **Define Critical Temperature**: - The critical temperature of a substance is the temperature above which it cannot be liquefied, regardless of the pressure applied. 2. **Compare Critical Temperatures**: - Ammonia (`NH3`) has a relatively high critical temperature, which allows it to be liquefied at ordinary temperatures. - Oxygen (`O2`), on the other hand, has a lower critical temperature, meaning it requires higher pressures or lower temperatures to be liquefied. 3. **Conclusion**: - Since `NH3` has a higher critical temperature, it can be liquefied easily at ordinary temperatures. In contrast, `O2` cannot be liquefied at ordinary temperatures due to its lower critical temperature. ### Final Answer: `NH3` can be liquefied at ordinary temperature without pressure because it has a higher critical temperature, whereas `O2` cannot be liquefied at ordinary temperature due to its lower critical temperature. ---
To understand why `NH3` (ammonia) can be liquefied at ordinary temperatures without the application of pressure, while `O2` (oxygen) cannot, we need to consider the concept of critical temperature. ### Step-by-Step Solution: 1. **Define Critical Temperature**: - The critical temperature of a substance is the temperature above which it cannot be liquefied, regardless of the pressure applied. 2. **Compare Critical Temperatures**: ...
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