Question

A sample of gaseous neon atoms at atmospheric pressure and $0^{\circ} \mathrm{C} \mathrm{con}$ tains $2.69 \times 10^{22}$ atoms per liter. The atomic radius of neon is 69 $\mathrm{pm} .$ What fraction of the space is occupied by the atoms themselves? What does this reveal about the separation between atoms in the gaseous phase?

Name: a sample of gaseous neon atoms at atmospheric pressure and 0circ mathrmc mathrmcon tains 269 times 1022 atoms per liter the atomic radius of neon is 69 mathrmpm what fraction of the space is occupie 2
Uploaded: 2021-08-29T02:17:25-08:00
Duration: 5 min 27 s
Channel: Christopher Dzorkpata
Description: a sample of gaseous neon atoms at atmospheric pressure and 0circ mathrmc mathrmcon tains 269 times 1022 atoms per liter the atomic radius of neon is 69 mathrmpm what fraction of the space is occupie 2

          A sample of gaseous neon atoms at atmospheric pressure and $0^{\circ} \mathrm{C} \mathrm{con}$
tains $2.69 \times 10^{22}$ atoms per liter. The atomic radius of neon is 69 $\mathrm{pm} .$
What fraction of the space is occupied by the atoms themselves? What
does this reveal about the separation between atoms in the gaseous phase?

Added by Brian E.

Chemistry Structure and Properties

Nivaldo J. Tro 1st Edition

Chapter 2

Instant Answer

Solved by Expert Christopher Dzorkpata

08/29/2021

Step 1

Given: Atomic radius of neon, $r = 69 \, \text{pm} = 69 \times 10^{-12} \, \text{m}$. Volume of a sphere, $V = \frac{4}{3} \pi r^3$. Substitute the radius value into the formula: $V = \frac{4}{3} \pi (69 \times 10^{-12})^3$. Calculate the volume occupied by one Show more…

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A sample of gaseous neon atoms at atmospheric pressure and $0^{\circ} \mathrm{C} \mathrm{con}$ tains $2.69 \times 10^{22}$ atoms per liter. The atomic radius of neon is 69 $\mathrm{pm} .$ What fraction of the space is occupied by the atoms themselves? What does this reveal about the separation between atoms in the gaseous phase?