What is the molar mass of a metal with a BCC | vedclass

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(D) For a $BCC$ structure, the number of atoms per unit cell is $Z = 2$. The formula for density is $d = \frac{Z \cdot M}{N_A \cdot a^3}$. Given: $d =

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$24.0 \ g \ mol^{-1}$

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(D) For a $BCC$ structure, the number of atoms per unit cell is $Z = 2$. The formula for density is $d = \frac{Z \cdot M}{N_A \cdot a^3}$. Given: $d = 10 \ g \ cm^{-3}$, $a = 200 \ pm = 200 	imes 10^{-10} \ cm = 2 	imes 10^{-8} \ cm$, and $N_A \approx 6.022 	imes 10^{23} \ mol^{-1}$. Substituting the values: $10 = \frac{2 	imes M}{6.022 	imes 10^{23} 	imes (2 	imes 10^{-8})^3}$. $10 = \frac{2 	imes M}{6.022 	imes 10^{23} 	imes 8 	imes 10^{-24}}$. $10 = \frac{2 	imes M}{4.8176}$. $M = \frac{10 	imes 4.8176}{2} = 24.088 \ g \ mol^{-1}$. Thus, the molar mass is approximately $24.0 \ g \ mol^{-1}$.

What is the molar mass of a metal with a $BCC$ structure having a density of $10 \ g \ cm^{-3}$ and an edge length of $200 \ pm$?

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