Final answer:
At standard conditions, equimolar samples of N₂ and O₂ would result in N₂ having a higher average molecular speed because of its lower molar mass compared to O₂.
Step-by-step explanation:
The molecular speeds of a gas are related to the temperature of the gas and the mass of its molecules. In general, at the same temperature, lighter molecules move faster than heavier molecules due to having less mass.
In the case of equimolar samples of N₂ and O₂ at standard conditions, O₂ has a higher molar mass compared to N₂ (32.0 g/mol for O₂ versus 28.0 g/mol for N₂).
Therefore, under the same conditions of temperature and pressure, the N₂ sample would have a higher average molecular speed than the O₂ sample because it has a lower molar mass, leading to higher average speeds according to the equations of kinetic molecular theory.