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(B) The molar mass $M$ is calculated as: $M = \frac{200 \, g}{24 	imes 10^{23} \, 	ext{atoms}} 	imes 6.022 	imes 10^{23} \, 	ext{atoms/mol} \appr

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$4.16$

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(B) The molar mass $M$ is calculated as: $M = \frac{200 \, g}{24 	imes 10^{23} \, 	ext{atoms}} 	imes 6.022 	imes 10^{23} \, 	ext{atoms/mol} \approx 50.18 \, g/mol$. For an $fcc$ unit cell, the number of atoms per unit cell $n = 4$. The edge length $a = 200 \, pm = 200 	imes 10^{-10} \, cm$. The volume $V = a^3 = (200 	imes 10^{-10} \, cm)^3 = 8 	imes 10^{-24} \, cm^3$. The density $ho = \frac{n 	imes M}{V 	imes N_A} = \frac{4 	imes 50.18}{8 	imes 10^{-24} 	imes 6.022 	imes 10^{23}} \approx 4.16 \, g/cm^3$.

An element crystallizes in an $fcc$ unit cell structure with an edge length of $200 \, pm$. If $200 \, g$ of the element contains $24 \times 10^{23}$ atoms, what is its density in $g/cm^3$?

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