On the magnitudes of molar volumes of real gases and ideal gases

(1) Standard conditions: refer to the state of 0°C and 1.01×10^5 Pa. The higher the temperature, the larger the volume ； The greater the pressure, the smaller the volume. Therefore, under non-standard conditions, its value is not necessarily “22.4L”. However, by simultaneously increasing the pressure and raising the temperature, or by reducing both the pressure and the temperature, the volume occupied by 1 mole of any gas can be 22.4 liters. 　　(2) For 1 mol of gas under non-standard conditions, its volume may be 22.4 L or it may not be 22.4 L. If the volume of the gas at room temperature (20°C, 1 atmosphere) is 24 L. 　 　　(3) The average distance between gas molecules is much larger than the diameter of the molecules; therefore, the volume of a gas is primarily determined by the average distance between these molecules. Under standard conditions, the average distance between molecules of different gases is almost equal; therefore, the molar volume of any gas under standard conditions is approximately 22.4 L/mol.

The molar volume of a gas is defined as “the volume occupied by one mole of a gas is called the molar volume of the gas.” That is, Vm = V/n. ”It can be seen from this that the molar volume of a gas is the ratio of the volume of the gas to its amount of substance at any temperature and pressure, whereas 22.4 L/mol is the molar volume of a gas under specific conditions (such as 0°C and 101 KPa). Note: When the temperature is above 0°C and the pressure is greater than 101 Kpa, the volume occupied by 1 mol of any gas can also be 22.4 L. Therefore, real gases can be considered ideal gases as long as they meet certain conditions. Thus, Avogadro’s law holds: \"At the same temperature and pressure, gases of the same volume contain the same number of molecules.\" In other words, under the same conditions, the average distance between molecules of different gases is almost equal.