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Number of atoms per unit cell (or type of cubic cell) from the mass of an atom and density x cell volume

The same question, asked 3 times: 21 Apr 2025 S1*, 21 Apr 2025 S2*, 25 Apr 2025 S1. Every wording below, oldest first.

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  1. Question 1

    21 Apr 2025 S1

    87
    The mass of an atom present in unit cell is 4.4×10−23 g4.4 \times 10^{-23}\ \mathrm{g} and the product of density and volume of unit cell is 1.792×10−22 g1.792 \times 10^{-22}\ \mathrm{g}. What is the type of cubic unit cell?

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  2. Question 2

    21 Apr 2025 S2

    80
    Calculate the number of atoms present per unit cell if product of density and volume of unit cell is 1.8×10−22 g1.8 \times 10^{-22}\ \mathrm{g}. [Mass of an atom =4.5×10−23 g= 4.5 \times 10^{-23}\ \mathrm{g}]

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  3. Question 3

    25 Apr 2025 S1

    56
    Calculate the number of particles present per unit cell if mass of a particle is 8.0×10−23 g[ρ×a3=3.2×10−22 g]8.0 \times10^{- 23}\text{ }g\left\lbrack \rho\times a^{3}= 3.2 \times10^{- 22}\text{ }g \right\rbrack

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