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Question
Anelement with molar mass 2.7× 10-2kg mol-1forms a cubic unit cell with edge length 405 pm. If its density is2.7 × 103 kg m−3,what is the nature of the cubic unit cell?
Anelement with molar mass 2.7× 10-2kg mol-1forms a cubic unit cell with edge length 405 pm. If its density is2.7 × 103 kg m−3,what is the nature of the cubic unit cell?
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Solution
Itis given that density of the element, d= 2.7 ×103 kgm−3
Molarmass, M = 2.7 ×10−2kg mol−1
Edgelength, a= 405 pm = 405 ×10−12m
=4.05 ×10−10m
Itis known that, Avogadro’s number, NA= 6.022 ×1023 mol−1
Applyingthe relation,
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Thisimplies that four atoms of the element are present per unit cell.Hence, the unit cell is face-centred cubic (fcc)or cubic close-packed (ccp).
Itis given that density of the element, d= 2.7 ×103 kgm−3
Molarmass, M = 2.7 ×10−2kg mol−1
Edgelength, a= 405 pm = 405 ×10−12m
=4.05 ×10−10m
Itis known that, Avogadro’s number, NA= 6.022 ×1023 mol−1
Applyingthe relation,
Thisimplies that four atoms of the element are present per unit cell.Hence, the unit cell is face-centred cubic (fcc)or cubic close-packed (ccp).
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