Which gas would occupy more volume at a constant temperature and pressure, 1.5 g of N2 gas or 1.5 g of O2 gas?A.N2 because there are more moles of N2.B.O2 because its molecules are larger.C.Neither gas occupies any volume.D.Both gases occupy equal volumes.
Question
Which gas would occupy more volume at a constant temperature and pressure, 1.5 g of N2 gas or 1.5 g of O2 gas?A.N2 because there are more moles of N2.B.O2 because its molecules are larger.C.Neither gas occupies any volume.D.Both gases occupy equal volumes.
Solution
According to Avogadro's law, equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. Therefore, the volume a gas occupies does not depend on the type of gas, but on the number of moles of the gas.
First, we need to calculate the number of moles for each gas.
The molar mass of N2 is approximately 28 g/mol and the molar mass of O2 is approximately 32 g/mol.
For N2: Number of moles = mass / molar mass = 1.5 g / 28 g/mol = 0.0536 mol
For O2: Number of moles = mass / molar mass = 1.5 g / 32 g/mol = 0.0469 mol
Even though N2 has more moles than O2, according to Avogadro's law, at the same temperature and pressure, both gases would occupy the same volume.
So, the answer is D. Both gases occupy equal volumes.
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