How many molecules of neon are associated with a 75⋅L volume of neon gas?

1 Answer
anor277
May 16, 2016

The question should have specified a temperature. I am going to assume that the gas is at room temperature, 298⋅K.

Explanation:

We know that at room temperature and pressure, 1 mol of ideal gas occupies a volume of 25.4⋅L.

We assume (reasonably) that Ne behaves ideally.

Thus the number of moles of Ne = 75⋅L25.4⋅L⋅mol−1 ≅ 3⋅mol.

But by definition, 1⋅mol of stuff possesses 6.022×1023 individual items of that stuff. If you can grasp this concept, it will save you a ton of angst.

Thus Molecules (atoms) of neon = 75⋅L25.4⋅L⋅mol−1×6.022×1023 neon atoms per mole

≅18×1023 neon atoms.

What is the mass of this quantity of neon gas?

(Neon gas is a monatomic molecule).

See also [here.](https://socratic.org/questions/what-is-the-mass-of-4-10-21-platinum-atoms)

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