A metal has a fcc lattice. The edge length of the unit cell is 404 pm. The density of the metal is 2.72 g cm3. The molar mass of the metal is (NA vogadro's constant = 6.02x 1023 mol-1).
40 g mol-1
30 g mol-1
27g mol-1
20 g mol-1
C.
27g mol-1
Given, cell is fcc, so Z = 4
Edge length, a= 404 pm= 4.04 x 10-8 cm
Density of metal, d= 2.72 g cm-3
NA = 6.02 x 1023 mol-1
Molar mass of the metal, M=?
We know that,
A compound is formed by cation C and anion A. The anions form hexagonal close packed (hcp) lattice and the cations occupy 75% of octahedral voids. The formula of the compound is :
C3A2
C3A4
C4A3
C2A3