Calculate the volume of the unit cell of an element having a molar mass of $27 \ g \ mol^{-1}$ that forms an $fcc$ unit cell. Given: $\rho \cdot N_{A} = 16.0 \times 10^{23} \ g \ cm^{-3} \ mol^{-1}$.
- A$7.50 \times 10^{-23} \ cm^3$
- B$6.75 \times 10^{-23} \ cm^3$
- C$5.75 \times 10^{-23} \ cm^3$
- D$8.25 \times 10^{-23} \ cm^3$
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An element crystallises in $fcc$ type of unit cell. The volume of one unit cell is $24.99 \times 10^{-24} \ cm^{3}$ and density of the element is $7.2 \ g \ cm^{-3}$. Calculate the number of unit cells in $36 \ g$ of a pure sample of the element.
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View SolutionSelect the $INCORRECT$ option regarding the cubic crystal system-
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