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Chemistry - Solid State Question with Solution | TestHub

ChemistrySolid StateCubic CrystalsMedium2 minPYQ_2017

ChemistryMediumsingle choice

A cubic unit cell of a metal with molar mass of $63.55 g mol^{- 1}$ has an edge length of 362 pm . Its density is $8.92 g cm^{- 3}$ . The type of unit cell is

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Answer:

Solution:

$Z Density = \frac{Z \times M}{a ^{3} \times N _{A}} = \frac{d \times N _{A} \times a ^{3}}{M} = \frac{8.92 \times 6.023 \times 1 0 ^{23} \times ( 362 \times 1 0 ^{- 10} ) ^{3}}{63.55} = 4$ $∴$ The metal crystallises in fcc.

Stream:JIPMERSubject:ChemistryTopic:Solid StateSubtopic:Cubic Crystals

⏱ 2mℹ️ Source: PYQ_2017

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