The density of chromium metal is 7.2 , g , cm | vedclass

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(B) The formula for density is $d = \frac{n 	imes M}{a^3 	imes N_A}$.Given:$d = 7.2 \, g \, cm^{-3}$$a = 289 \, pm = 289 	imes 10^{-10} \, cm$$M =

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$BCC$

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(B) The formula for density is $d = \frac{n 	imes M}{a^3 	imes N_A}$.Given:$d = 7.2 \, g \, cm^{-3}$$a = 289 \, pm = 289 	imes 10^{-10} \, cm$$M = 52 \, g \, mol^{-1}$$N_A = 6.02 	imes 10^{23} \, mol^{-1}$Rearranging for $n$:$n = \frac{d 	imes a^3 	imes N_A}{M}$$n = \frac{7.2 	imes (289 	imes 10^{-10})^3 	imes 6.02 	imes 10^{23}}{52}$$n = \frac{7.2 	imes 2.41 	imes 10^{-23} 	imes 6.02 	imes 10^{23}}{52}$$n = \frac{7.2 	imes 2.41 	imes 6.02}{52} \approx 2$Since the number of atoms per unit cell $n = 2$, the unit cell is $BCC$ (Body-Centered Cubic).

The density of chromium metal is $7.2 \, g \, cm^{-3}$. If the edge length of the unit cell is $289 \, pm$, determine the type of unit cell (Simple Cubic, Body-Centered Cubic, or Face-Centered Cubic). [Atomic mass of $Cr = 52 \, a.m.u.$, $N_A = 6.02 \times 10^{23} \, mol^{-1}$]

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