At the same temperature and pressure, which sample contains the samenumber of moles of particles as 1 liter of o2() 1 l ne(g) (3) 0.5 l so2(g)(2) 2 l n2(g) (4) 1 l h2o(ℓ)

1 L of Ne (g)

Explanation:

According to the ideal gas law, . Rearranging this expression for moles, we would get:

For two samples, the following equation should then hold:

At the same temperature and pressure, this is then rearranged to:

Since we're examining the moles of particles rather than moles of molecules, we may use stoichiometry assuming that the first gas has x atoms in a molecule and that the second gas has y atoms in a molecule:

Assuming that the first gas is oxygen, we get:

Given a total of 1 liter:

None of the options gives the same number of moles of atoms. However, thinking about molecules, it is sufficient to state that:

This means 1 liter of neon would have the same number of molecules as 1 liter of oxygen.