Calculate the mass of a $bcc$ unit cell if the metal has a molar mass of $56 \ g \ mol^{-1}$.
- A$1.86 \times 10^{-22} \ g$
- B$9.3 \times 10^{-24} \ g$
- C$2.79 \times 10^{-24} \ g$
- D$3.72 \times 10^{-22} \ g$
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An element with density $2.8 \ g \ cm^{-3}$ forms an $fcc$ unit cell having an edge length of $4 \times 10^{-8} \ cm$. Calculate the molar mass of the element.
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Metal $M$ crystallises in $fcc$ lattice. If the unit cell has an edge length of $4.077 \ \mathring{A}$ and the density is $10.5 \ g \ cm^{-3}$,then the atomic weight of the metal is:
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View SolutionThe formula for the determination of the density of a unit cell is:
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