an element having atomic nmass 60.2 has a face center cubic unit cell the edgelemgth of the unit cell is 100 pm find out density of the element
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answer- d≈.62×10^7
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Answer:
Given = atomic mass = 60.2
FCC (length)= 100pm= 100 x 10⁻¹⁰
to find = density
solution =
density of unit cell = mass of unit cell / volume of unit cell
mass of unit cell = no.of atoms in the unit cell x mass of each atom
mass of unit cell = 4 x 60 /6.023 x 10²³
no. of atoms in FCC unit cell = 8 x 1/8 ++ 6 x 1/2 = 4
volume of the unit cell = (100 x 10⁻¹⁰)³= 10 x 10⁻²⁴
so put this value in above formula ,
=4 x60 / 6.023 x 10²³ x 10 x 10⁻²⁴
=240 / 6.023 x 10²³ x 10 x 10⁻²⁴
0.25g/cm³
so the final density will be 0.25g/cm³
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