Final answer:
One mole of any gas occupies a volume of 22.4 liters at standard temperature and pressure (STP), which is 0°C and 1 atm pressure. This is a fact widely used in stoichiometry and to understand gas behavior under these specific conditions.
Step-by-step explanation:
The volume that one mole of any gas occupies at room temperature and normal pressure is a concept that is defined under specific conditions known as standard temperature and pressure (STP), which is 0°C and 1 atm pressure. According to the ideal gas law, one mole of any gas at STP occupies a volume of 22.4 liters. This constant volume is based on Avogadro's hypothesis, which states that equal volumes of all gases at the same temperature and pressure contain the same number of molecules.
The molar volume is a useful conversion factor in stoichiometry problems, but only when the conditions are at STP. If conditions differ from STP, the combined gas law may be used to calculate what the volume would be under standard conditions. For instance, 2 moles of hydrogen gas would occupy 44.8 liters at STP, reflecting that the molar volume scales directly with the amount of substance.
STP conditions are important in chemistry calculations because molar volume allows chemists to easily convert between moles and volume for gases. This can be extremely useful in understanding chemical reactions and processes involving gaseous substances.