Which of the following is true about the behavior of gases at STP?

At standard temperature and pressure (STP), which is defined as 0 degrees Celsius (273.15 K) and 1 atm pressure, one mole of any ideal gas occupies a volume of 22.4 liters. This is derived from the ideal gas law, which states that under these specific conditions, the behavior of gases can be approximated as ideal. Therefore, all gases, regardless of their molecular weight or identity, occupy this same volume when evaluated at STP, exemplifying the fundamental principle of gas behavior.

The notion that all gases occupy the same volume highlights the essence of the ideal gas law, where the properties of the gas are considered collectively instead of individually. This principle supports the idea that the volume occupied is a function of temperature and pressure, rather than the characteristics of the individual gas itself.

The other options touch on significant aspects of gas behavior, but they do not align with the established characteristics of gases at STP. The variation in gas volume based on molecular weight, the notion that gases do not follow ideal gas laws, and the behavior under increased pressure all pertain to conditions that deviate from ideal behavior, but they do not apply specifically to gases at STP. The behavior of gases at STP is a cornerstone