If 5.00 g of gas A and 5.00 g of gas B are mixed in the same container, and the partial pressure of gas B is determined to be twice that of gas A, what do we know about the gases?

Question

27-10-2023
Chemistry

High School

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If 5.00 g of gas A and 5.00 g of gas B are mixed in the same container, and the partial pressure of gas B is determined to be twice that of gas A, what do we know about the gases?

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MattZayn7 MattZayn7 · Answer 1 · 2024-11-04T06:33:46-05:00

When 5.00 g each of gas A and B are mixed and gas B's partial pressure is twice that of gas A, it indicates that gas B has a lower molar mass and thus more moles than gas A in the container.

If 5.00 g of gas A and 5.00 g of gas B are mixed in the same container, and the partial pressure of gas B is twice that of gas A, what we know is that the molar mass of gas B is likely to be lower than that of gas A. This can be deduced from the ideal gas law (PV=nRT) when applied to each gas separately, considering that the gases behave independently and the total pressure in the container is the sum of their individual pressures.

Since the masses of the two gases are equal, and the volume and temperature are constants, the difference in pressure must stem from the number of moles of each gas. The gas with the lower molar mass will have more moles, hence a higher partial pressure.

For example, if the total pressure of the gases mixed is 1 atm and gas B has a pressure twice that of gas A, then the partial pressure of A would be 0.5 atm. Gas B, with twice the partial pressure of gas A, would be 1 atm. This implies gas B has more moles than gas A because the partial pressure of a gas is proportional to the number of moles.