Given the atomic radius of neon, 0.69 å, and knowing that a sphere has a volume of 4πr3/3, calculate the fraction of space that ne atoms occupy in a sample of neon at stp.

Question

Carley Solomon

Chemistry

4 February, 14:08

Given the atomic radius of neon, 0.69 å, and knowing that a sphere has a volume of 4πr3/3, calculate the fraction of space that ne atoms occupy in a sample of neon at stp.

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Answers (1)

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Semaj Kaiser · Answer 1

First, compute the volume of one atom by means of the spherical volume formula given: 4pi (.69) ^3/3. You should get 1.376 A^3. One angstrom (A) cubed is about 1 x 10^-27 liters. Multiply and get a atomic volume of 1.376 x 10^-27 L. That is the volume of only one atom. Multiply this volume by 6.02 x 10^23 (Avogadro s Number) to get the total volume of the atoms. You should get 8.284 x 10^-4 L. Now that we have our total volume for our atoms in liters, divide that number by volume of any ideal gas at STP, which is 22.4 L according to my text. You should get a final answer of 3.7 x 10^-5.