An element has an fcc structure. If 200 g of | vedclass

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(B) $1$. Calculate the volume of the unit cell using the density formula: $ho = \frac{Z 	imes M}{N_A 	imes a^3}$.$2$. First, find the molar mass $

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$299.9 \ pm$

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(B) $1$. Calculate the volume of the unit cell using the density formula: $ho = \frac{Z 	imes M}{N_A 	imes a^3}$.$2$. First, find the molar mass $(M)$: $M = \frac{	ext{mass} 	imes N_A}{	ext{number of atoms}} = \frac{200 \ g 	imes 6.022 	imes 10^{23} \ mol^{-1}}{4.12 	imes 10^{24}} \approx 29.23 \ g \ mol^{-1}$.$3$. For $fcc$ structure, $Z = 4$.$4$. Rearrange the density formula for $a^3$: $a^3 = \frac{Z 	imes M}{ho 	imes N_A} = \frac{4 	imes 29.23}{7.2 	imes 6.022 	imes 10^{23}} \approx 2.697 	imes 10^{-23} \ cm^3$.$5$. Calculate $a$: $a = \sqrt[3]{2.697 	imes 10^{-23}} \approx 2.999 	imes 10^{-8} \ cm = 299.9 \ pm$.

An element has an $fcc$ structure. If $200 \ g$ of this element contains $4.12 \times 10^{24}$ atoms and the density of the element is $7.2 \ g \ cm^{-3}$, calculate the edge length of the unit cell.

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