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A metal crystallizes into cubic phases, face centered cubic (BCC), whose unit cell lengths are 3.5 and 3.0 Å, respectively, Calculate the ratio of densities of FCC and BCC.

Shane Macguire , 11 Years ago
Grade upto college level
anser 1 Answers
Deepak Patra

Last Activity: 11 Years ago

Hello Student,
Please find the answer to your question
Density in fcc = n1 * at.wt./V1 *No.
Density in bcc = n2 * at.wt./V2 *No.
fcc unit cell length = 3.5 Å
bcc unit cell length = 3.0 Å
Density in fcc = n1 * at.wt./V1 *Av.No.
Density in bcc = n2 * at.wt./V2 *Av.No.
∴ Dfcc/Dbcc = n1/n2 * V2/V1
n1 for fcc = 4; Also V1 = a3 = (3.5 * 10-8)3
n2 for fcc = 2; Also V2 = a3 = (3.0 * 10-8)3
∴ Dfcc/Dbcc = 4 * (3.0 * 10-8)3/2 * (3.5 * 10-8)3 = 1.259

Thanks
Deepak patra
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