An element crystallizes in a structure having fcc unit cell of an edge length equal to 200 pm . Calculate the density (in g cm−3) if 100 g of this element contains 12×1023 atoms.
A
41.66
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
B
4.166
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
10.25
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
1.025
No worries! We‘ve got your back. Try BYJU‘S free classes today!
Open in App
Solution
The correct option is A41.66 As 12×1023 atoms have a mass of 100 g, 6×1023 atoms have mass of 50 gm and so, the molar mass is 50 g/mol.
The formula for density is as follows:
d=ZMVNA=4×50(200×10−10)3×6×1023=41.66 g cm−3
where Z=4 because the element crystallizes is fcc structure.