Asked by Sunny
An element has ccp packing with a face-centered cubic unit cell. Its density is 1540 kg/m3 and the unit cell volume is 1.73 x 10-22 cm3. Calculate the molar mass (g/mol) of the element to three significant figures.
CCP: cubic close pack
CCP: cubic close pack
Answers
Answered by
DrBob222
You have the density (1.54 g/cc) and the volume of the unit cell (1.73 x 10^-22 cc). From mass = volume x density you can calculate mass of atoms in one unit cell. Then you know [(4 atoms/unit cell x molar mass)/6.02 x 10^23] = mass atoms. You may want to check Avogadro's number to three s.f.
Determine molar mass from this.
Determine molar mass from this.
Answered by
Sunny
The 4 atoms.unit cell is where I got confused. How do you know that? And how does it change for hexagonal close pack and body centered cubic?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.