Question

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.

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.

Answer 2

Answer:

The volume of Neon would be 15290811,94 pm^3

Explanation:

In order to solve this we just have to calculate the volume that the neon will occupy, its radius is 0,69 A or 154 pm with this we just have to calculate with the next formula:$Volume: \frac{4r^3\pi }{3} \\Volume: \frac{4(154^3pm*3,14 }{3}\\Volume: 15290811,94 pm^3$

So the volume of Neon would be 15290811,94 pm^3