Answer to Question #219362 in General Chemistry for Olivia Hughes

Question #219362

 Xenon crystallizes in a FCC unit cell. If we assume xenon has a radius of 186.9 pm, what is the density of xenon in g/cm3 ?


1
Expert's answer
2021-07-26T06:34:08-0400

Number of atoms present in a FCC unit are four.

Density of face-centered cubic unit cell=4×MA3×Na\frac{4\times M}{A3\times Na}

M=molar mass of xenon=131.293gM=molar\space mass \space of \space xenon=131.293g

A=A= edge of unit cell=22r=2×2×186.9×1012=3.8668×103cm=2\sqrt{2r}=2\times \sqrt{2\times 186.9\times 10^{-12}}=3.8668\times 10^{-3}cm

Na=Na= Avogadro's number=6.02×1023=6.02\times 10^{23}

In this case, density of xenon=4×131.293g(3.8668×103)3×6.02×1023cm3=525.172g(3.4806×1016cm3)=1.5089×1014g/cm3=\frac{4\times 131.293g}{(3.8668\times 10^{-3})^3 \times 6.02\times 10^{23}cm^3}=\frac{525.172g}{(3.4806\times 10^{16}cm^3)}=1.5089\times 10^{-14}g/cm^3


Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be the first!

Leave a comment