what is the mass of aluminum? d= 4.05 g/cm3

Chemistry
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in a face-centered cubic unit cell, aluminum is crystallized. the density of aluminum is 4.05 g/cm3. what is the mass, g of aluminum in the unit cell?

Sep 8th, 2015

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http://genchem1.chem.okstate.edu/1515F01/ProblemSet/1515F01PS3Ans.pdf

http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch13/unitcell.php

please use the links above to get more knowledge

From the website above we know that there are 8 Al atoms in every unit cell.

So to find the mass of Al in the unit cell, we need to find the mass of an Al atom (in grams) and multiply it by eight.

1 atom  x  (27.0 g / 6.02 x 1023 atoms  = mass of 1 Al atom in grams

Then, since there are 8 atoms in a face centered unit cell:
  8 atoms   x   (mass of 1 Al atom in grams)  =  mass of Al atoms in one unit cell

Since we know the density of aluminum and we know the mass of a unit cell, we can calculate the volume of the unit cell using the density formula:
                      Density = mass/ volume      
                      4.16 g  = mass of Al atoms in a unit cell / volume in cm3

I am still doing the calculations I will supplement the answer



Please let me know if you need any clarification. I'm always happy to answer your questions.
Sep 8th, 2015

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