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Calculate the molar mass of metal having density $22.24 \mathrm{~g} \mathrm{~cm}^{-3}$, crystallizes to form unit cell containing 4 particles.
$\left(\mathrm{a}^3=5.6 \times 10^{-23} \mathrm{~cm}^3\right)$
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$\left(\mathrm{a}^3=5.6 \times 10^{-23} \mathrm{~cm}^3\right)$
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Verified Answer
The correct answer is:
$187.4 \mathrm{~g} \mathrm{~mol}^{-1}$
$\mathrm{d}=\frac{\mathrm{Z} \times \mathrm{M}}{\mathrm{V} \times \mathrm{N}_{\mathrm{A}}}=\frac{4 \times \mathrm{M}}{5.6 \times 10^{-23} \times 6.02 \times 10^{23}}$
or $22.24=\frac{4 \times M}{5.6 \times 6.02}$
$\mathrm{M}=187.43 \mathrm{~g} / \mathrm{mol}$
or $22.24=\frac{4 \times M}{5.6 \times 6.02}$
$\mathrm{M}=187.43 \mathrm{~g} / \mathrm{mol}$
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