Assuming all gases behave ideally, which of the following gases would occupy the largest volume at 25oC and 101.325 kPa? 25 g of Ar(g) 25 g of He(g) 25 g of H2(g) 25 g of O2(g) 25 (g) of F2(g)

To answer this question, we need to use the Ideal Gas Law, which states that the volume of a gas is directly proportional to the number of moles of the gas. The formula for the Ideal Gas Law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

The number of moles of a gas can be calculated using the formula n = m/M, where m is the mass of the gas and M is the molar mass of the gas.

Given that the mass of each gas is 25 g, we can calculate the number of moles for each gas:

1. Ar(g): M = 39.95 g/mol, so n = 25 g / 39.95 g/mol = 0.626 moles
2. He(g): M = 4.00 g/mol, so n = 25 g / 4.00 g/mol = 6.25 moles
3. H2(g): M = 2.02 g/mol, so n = 25 g / 2.02 g/mol = 12.38 moles
4. O2(g): M = 32.00 g/mol, so n = 25 g / 32.00 g/mol = 0.781 moles
5. F2(g): M = 38.00 g/mol, so n = 25 g / 38.00 g/mol = 0.658 moles

From these calculations, we can see that H2(g) has the highest number of moles. Therefore, according to the Ideal Gas Law, H2(g) would occupy the largest volume at 25oC and 101.325 kPa.