An element (atomic mass = 100 g/mol) that has a bcc structure has a unit cell edge length of 400 pm. The density of the element is: (Take NA=6×1023)
A
10gcm−3
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B
5.2gcm−3
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C
7.2gcm−3
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D
2.1gcm−3
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Solution
The correct option is B5.2gcm−3 Density ρ is given by ρ=ZMa3×NA Since it has a BCC structure, Z=2 ∴ρ=2×100(400)3×6×1023×10−30 ⇒ρ=2×100(4)3×6×10−1 ≈5.2g/cm−3