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 ~cm ⁻³ . The molar mass of the metal is ( N_A Avogadro's constant =6.02 10²³ ~mol ⁻¹ )

Step-by-step solution

Given, cell is fcc, so Z=4 Edge length, a=404 pm =4.04 10⁻⁸ ~cm Density of metal, d=2.72 ~g ~cm ⁻³N_A=6.02 10²³ ~mol ⁻¹ Molar mass of the metal, M= ? We know that density, d= Z M 2^3 N_A aligned M & = d a^3 N_A Z & = 2.72 (4.04 10⁻⁸ )^3 6.02 10²³ 4 & =27 ~g ~mol ⁻¹ aligned