Calculate the molar mass of an element if it forms $fcc$ unit cell structure. [Mass of unit cell $= 1.8 \times 10^{-22} \ g$,$N_A = 6.022 \times 10^{23} \ mol^{-1}$]
- A$27.0 \ g \ mol^{-1}$
- B$24.4 \ g \ mol^{-1}$
- C$21.0 \ g \ mol^{-1}$
- D$30.2 \ g \ mol^{-1}$
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View SolutionAn 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.
Calculate the number of atoms present in a unit cell of an element having molar mass $190 \ g \ mol^{-1}$ and density $20 \ g \ cm^{-3}$. Given that $[a^3 \cdot N_A = 38 \ cm^3 \ mol^{-1}]$.
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