Calculate the atomic mass of an element having cubic structure with one atom at each corner. The volume of the unit cell is `2.4xx10^(-23) cm^3` and density is `4.4 g cm^(-3`.

Calculate the atomic mass of an element which crystallises into a cubic structure with one atom on each corner of the cube. The volume of the unit cell is 24xx10^-24 cm^3 and density is 7.2 gcm^-3 .

An element crystallises' into a, structare which may be described by a cubic type of unit celt having one atom on each C0rner of the cube and two atoms on one of its diagonals. If yolume of this unit cell is 24x 10^-(24) cm^3 and density of element is 7.2 g / cm^-3 . calculate the number of atoms present in 200 g of the element .

Calculate the number of atoms in a cubic based unit cell having one atom on each Corner and two atoms on each body diagonal

Calculate the number of atoms present in 1.4 g of N_2 molecule.

CsCl forms unit cells in which caesium ions are in contact with each other and chloride ions occupy the body centre. If the volume of a unit cell of CsCl is 7.014xx10^(-23)cm^(3) , the Cs - Cs distance is nearly

A metal of atomic mass 60u has a body centred cubic lattice. The edge length of the unit cell is 286 pm. Calculate the atomic radius and the density of the metal.

An element has a body centred cubic structure with a cell edge of 288 pm. The density of the element is 7.2 g/ cm^3 . How many atoms are present in 208 g of the element?