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A cubic unit cell of a metal with molar mass of $63.55 \mathrm{~g} \mathrm{~mol}^{-1}$ has an edge length of 362 pm . Its density is $8.92 \mathrm{~g} \mathrm{~cm}^{-3}$. The type of unit cell is
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$\begin{aligned}& \text { Density }=\frac{Z \times M}{a^3 \times N_A} \\Z & =\frac{d \times N_A \times a^3}{M} \\
& =\frac{8.92 \times 6.023 \times 10^{23} \times\left(362 \times 10^{-10}\right)^3}{63.55}=4\end{aligned}$
$\therefore$ The metal crystallises in fcc.
& =\frac{8.92 \times 6.023 \times 10^{23} \times\left(362 \times 10^{-10}\right)^3}{63.55}=4\end{aligned}$
$\therefore$ The metal crystallises in fcc.
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