Calculate the density of a metal with molar m | vedclass

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(D) The density $(d)$ of a unit cell is given by the formula: $d = \frac{Z 	imes M}{a^3 	imes N_{A}}$For a $bcc$ structure, the number of atoms per

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$7.8$

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(D) The density $(d)$ of a unit cell is given by the formula: $d = \frac{Z 	imes M}{a^3 	imes N_{A}}$For a $bcc$ structure, the number of atoms per unit cell $(Z)$ is $2$.The molar mass $(M)$ is $56 \ g \ mol^{-1}$.The edge length $(a)$ is $288 \ pm = 288 	imes 10^{-10} \ cm$.Avogadro's number $(N_{A})$ is $6.022 	imes 10^{23} \ mol^{-1}$.Substituting the values:$d = \frac{2 	imes 56}{(288 	imes 10^{-10} \ cm)^3 	imes 6.022 	imes 10^{23} \ mol^{-1}}$$d = \frac{112}{2.3887 	imes 10^{-23} 	imes 6.022 	imes 10^{23}}$$d = \frac{112}{14.385} \approx 7.78 \ g \ cm^{-3}$

Calculate the density of a metal with molar mass $56 \ g \ mol^{-1}$ that crystallises in a $bcc$ structure with an edge length of $288 \ pm$. (in $g \ cm^{-3}$)

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