The quantity that can differ between the two gases is:
the mass of each gas.
Since the gases are at the same pressure, volume, and temperature, their behaviors can be described by the ideal gas law (\(PV = nRT\)), where \(n\) is the number of moles, and \(R\) is the gas constant. The mass of the gas will depend on the molar mass of each gas, so it is possible for the masses to differ even if the other conditions are the same.
The number of moles could also differ depending on the molar mass, so that one gas could have more or fewer moles; however, the question specifically asks about the mass. The gas constant \(R\) is specific to each gas but does not change in this context as the conditions are the same. The molar volume is also constant for ideal gases under the same conditions and pressure.
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