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Question

A metal has a fcc lattice. The edge length of the cell is 404 pm. The density of the metal is 2.72 g cm3 . The molar mass of the metal is
(NA Avogadro's constant = 6.02×1023mol1)


A

27 g mol1

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B

20 g mol1

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C

40 g mol1

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D

30 g mol1

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Solution

The correct option is A

27 g mol1


For fcc, Z=4

Note: We will convert all units to cm from m, this is an important step as density is given in g/cc. This will take care of the units of molar weight as well - g/mol.
d=ZMNAa3M=d×NA×a3Z=2.72×6.023×1023×(404×1010)34M=26.9927 g mol1


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