A given gas varies in its physical properties over a wide range of temperatures. The various such variations in the properties must be observed at specific temperatures. The discussion about the temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is one such example.
Complete step by step answer:
The different types of temperature given above have their own significance. In order to understand which one fits the question given to us, it is important that we discuss all of them.
-Every vapour or gas the tendency to liquefy. The conditions at which this liquefaction occurs is directly dependent on the pressure and temperature of the vapor. The various conditions possible for liquefaction can be tuned according to the various permutations of temperature and pressure. But because of physical limits, there exists a certain temperature value beyond which liquefaction is not possible, irrespective of variations in the pressure. That temperature is known as Critical Temperature.
Real gases that are observed by us do not behave like ideal gases at all conditions. But at a certain temperature, these real gases start behaving like ideal gases over a certain range of pressure. This temperature is known as Boyle’s temperature.
Inversion temperature is the temperature at which the sign for Joule-Thomson effect with regards to a gas gets changed. At this point, the expansion of the gas is not allowed to be either cooled or heated without expending energy.
Hence, Option B is the correct option.
At Boyle’s temperature, real gases behave like ideal gases. This indirectly means that all assumptions that we consider for an ideal gas, hold true for the real gas at this temperature.