A metal crystallises in bcc lattice with unit | vedclass

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(A) Given, metal crystallises in $bcc$ lattice, therefore $Z = 2$. Edge length $a = 300 \ pm = 300 	imes 10^{-10} \ cm$. Density $d = 6.15 \ g \ cm^{

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$50 \ g \ mol^{-1}$

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(A) Given, metal crystallises in $bcc$ lattice, therefore $Z = 2$. Edge length $a = 300 \ pm = 300 	imes 10^{-10} \ cm$. Density $d = 6.15 \ g \ cm^{-3}$. Using the formula for density: $d = \frac{Z 	imes M}{a^3 	imes N_A}$. Rearranging for molar mass $M$: $M = \frac{d 	imes a^3 	imes N_A}{Z}$. Substituting the values: $M = \frac{6.15 	imes (300 	imes 10^{-10})^3 	imes 6.022 	imes 10^{23}}{2}$. $M = \frac{6.15 	imes 27 	imes 10^{-24} 	imes 6.022 	imes 10^{23}}{2} = \frac{99.965}{2} \approx 49.98 \ g \ mol^{-1}$. Thus, the molar mass is approximately $50 \ g \ mol^{-1}$.

$A$ metal crystallises in $bcc$ lattice with unit cell edge length of $300 \ pm$ and density $6.15 \ g \ cm^{-3}$. The molar mass of the metal is

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