Final answer:
The mass and number of air molecules in a container can be calculated with the volume of the container and the average molar mass of air, using the fact that one mole of an ideal gas occupies 22.4 L at STP.
Step-by-step explanation:
The mass of air and the number of air molecules in a container can be calculated using the ideal gas law and the molar mass of air.
Given the average molar mass of air as 29 g/mol and knowing that the molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 liters per mole, we can use the volume of the container to calculate the number of moles contained.
For example, if a living room has dimensions of 5 m × 5 m × 3 m, the volume of air in the room is 75 m³.
Converting this volume to liters (1 m³ = 1000 L), we get 75,000 liters.
The mass of one mole of air is 29 g, so the mass of air in the room can be calculated by converting moles to grams using this molar mass.
If we know that at STP, one mole of an ideal gas occupies 22.4 L, we then calculate the
number of moles by dividing the volume of the room in liters by 22.4 L/mol.
Q: How many air molecules are in the container, and what is the mass of that air?