Final answer:
The value for molar gas volume at STP is not dependent on the identity of the gas; it is 22.4 liters for all ideal gases. This is according to the ideal gas law, which holds true under standard conditions, despite slight deviations in real gases represented by the compressibility factor.
Step-by-step explanation:
The statement that the accepted value for molar gas volume varies based on the identity of the gas is false. In chemistry, the molar volume of a gas is defined as the volume occupied by one mole of a gas.
At Standard Temperature and Pressure (STP), which is 0°C and 1 atmosphere of pressure, all ideal gases have a molar volume of 22.4 liters. This is based on the ideal gas law, PV = nRT, where P is the pressure, V is the volume, T is the temperature, n is the number of moles, and R is the universal gas constant.
However, real gases do show deviations from ideal behavior due to their molecular volume and intermolecular interactions. The compressibility factor (Z) provides a measure of how much a real gas deviates from ideal behavior by comparing the molar volume of an actual gas to the molar volume of an ideal gas at the same conditions.
Despite these deviations, the molar volume of a gas at STP is a useful concept for carrying out stoichiometric calculations and is generally used for practical purposes because under most conditions, real gases behave similarly to ideal gases.