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Number of atoms in a given mass of a metal from its unit cell data

This type of question, asked 10 times: May 2022 S1, 4 May 2023 S2, 19 Apr 2025 S1, 22 Apr 2025 S2, 23 Apr 2025 S1, 15 Apr 2026 S2, 16 Apr 2026 S1, 17 Apr 2026 S2, 18 Apr 2026 S1, 13 May 2026 S1. All 10 questions below, oldest first.

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  1. Question 1

    May 2022 S1

    92
    Calculate the number of atoms in 5-gram metal that crystallises to form simple cubic unit cell structure having edge length 336 pm. (Density of metal = 9.4 g cm−3^{-3})

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  2. Question 2

    4 May 2023 S2

    71
    Calculate the number of atoms in 0.3-gram metal if it forms bcc structure. ρ×a3=3×10−22\rho\times a^3 = 3\times10^{-22} g

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  3. Question 3

    19 Apr 2025 S1

    94
    Calculate the number of atoms present in 1.58 g metal if it forms bcc structure.
    [ρ×a3=1.58×10−22 g]\left\lbrack \rho\times a^{3}= 1.58 \times10^{- 22}\text{ }g \right\rbrack

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  4. Question 4

    22 Apr 2025 S2

    77
    Calculate the number of atoms present in 1 g of an element if it forms fcc unit cell structure. [ρ×a3=6.8×10−22 g]\left\lbrack \rho \times a^{3}= 6.8 \times10^{- 22}\text{ }g \right\rbrack

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  5. Question 5

    23 Apr 2025 S1

    55
    Calculate the number of atoms in 1g1g metal if it forms fcc crystal structure. [ρ×a3=1.728×10−22 g]\left\lbrack \rho\times a^{3}= 1.728 \times10^{- 22}\text{ }g \right\rbrack

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  6. Question 6

    15 Apr 2026 S2

    20
    Calculate the number of atoms present in 1.625 g metal if it forms bcc unit cell structure. [ρ×a3=3.25×10−22[\rho \times a^3 = 3.25 \times 10^{-22} g]]

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  7. Question 7

    16 Apr 2026 S1

    22
    Calculate the number of atoms present in 90 g of metal if it forms bcc structure. [ρ×a3=1.8×10−22[\rho \times a^3 = 1.8 \times 10^{-22} g ]

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  8. Question 8

    17 Apr 2026 S2

    19
    Calculate the number of atoms in 1 g metal that forms bcc crystal structure [ρ×a3=6.6×10−22 g][\rho \times a^3 = 6.6 \times 10^{-22}\ \mathrm{g}]

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  9. Question 9

    18 Apr 2026 S1

    19
    Calculate the number of atoms present in 11 g metal that forms simple unit cell structure if product of density and volume of unit cell is 66.5×10−2466.5 \times 10^{-24} g

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  10. Question 10

    13 May 2026 S1

    19
    Calculate the number of atoms in 0.60.6 g metal that forms bcc structure having density 8.5 g cm−38.5\ \mathrm{g\,cm^{-3}}, if the volume of unit cell is 3.6×10−23 cm33.6 \times 10^{-23}\ \mathrm{cm^3}

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