At STP, how many liters of oxygen gas (O2) are required to react completely with 2 moles of hydrogen gas (H2) to form water (H2O)?

To determine the volume of oxygen gas (O2) required to react completely with 2 moles of hydrogen gas (H2) to form water (H2O), we can use the balanced chemical equation for the reaction between hydrogen and oxygen to produce water:
2H2 (g) + O2 (g) -> 2H2O (g)
According to the balanced equation, two moles of hydrogen gas react with one mole of oxygen gas to produce two moles of water vapor. Since we have 2 moles of hydrogen gas, we need half as many moles of oxygen gas to react completely. Therefore, we need 1 mole of oxygen gas (O2) for this reaction. Now, at standard temperature and pressure (STP), one mole of any ideal gas occupies a volume of approximately 22.4 liters. So, 1 mole of oxygen gas (O2) at STP occupies 22.4 liters. Therefore, to react completely with 2 moles of hydrogen gas, we would need 22.4 liters of oxygen gas at STP.