24.04 (Sample A)16.81 (Sample B) Both Sample a and b are the number of atoms in aluminum foil.the volumes:2.40cm^3 (Sample A)1.62cm^3 (Sample B)Based on the given information above, calculate the volume of 1.00 atom of aluminum in both of the samplesaverage the two volumes.Also given: the density of aluminum is 2.702g/cm^3With the average of the two volumes, using hte general atomic shape as spherical and the forumula for the volume of a sphere, calculate the radius if 1.00 atom of Aluminum in cm^3 where V 4/3 quot;piequot; r^3Express the above radius in Angstroms(Hint: Aluminum is found to be 2.864 Angstroms1 Angstrom 10^-8cmOne atom of Aluminum has a diameter of 2.864 x 10^-8cm.Calculate the experimental diameter from the radius.
I don't understand how you can have 16.81 atoms of aluminum in a sample of aluminum foil.
