A metal (atomic mass = 50 ) has a body centred cubic crystal structure. If the density of the metal is 5.96 g `cm^(-3)`, calculate the volume of the unit cell.

A metal (atomic mass = 40) has a body centred cubic crystal structure. If the density of the metal is 4.50 g cm^(-3) , calculate the volume of the unit cell.

A metal (atomic mass = 40) has a body centred cubic crystal structure. If the density of the metal is 4.50 g cm^(-3) , calculate the volume of the unit cell.

A metal (atomic mass = 50) has a body centred cubic crystal structure. The density of the metal is 5.96 g cm^(-3) . Find the volume of this unit cell.

Density of a unit cell is the same as the density of the substance. So, if the density of the substance is known, we can calculate the number of atoms or dimensions of the unit cell. The density of the unit cell is related to its formula mass (M), number of atoms per unit cell (z), edge length (a in cm), and Avogadro's constant N_(A) , as rho=(zxxM)/(a^(3)xxN_(A)) Q. A metal A (atomic mass=60) has a body-centred cubic crystal structure. the density of the metal is 4.2 g cm^(-3) . the volume of unit cell is

Density of a unit cell is same as the density of the substance. If the density of the substance is known, number of atoms or dimensions of the unit cell can be calculated . The density of the unit cell is related to its mass(M), no. of atoms per unit cell (Z), edge length (a in cm) and Avogadro number N_A as : rho = (Z xx M)/(a^3 xx N_A) A metal X (at. mass = 60) has a body centred cubic crystal structure. The density of the metal is 4.2 g cm^(-3) . The volume of unit cell is

A metal X ( at. Mass = 60) has a body centred cubic crystal structure. The density of the metal is 4.2 g cm^(-3) . The volume of unit cell is