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?

An element having atomic mass '52,' occurs in bcc structure with a cell edge of 288 pm. The density of the element is '7.2 gcm^-3'. Evaluate Avogadro number.

An element of density 7.2 g cm^(-3) occurs in bcc structure with unit cell edge of 280 pm. Calculate molecular mass of the element and number of atoms present in 100 g of the element.

An element ‘A’ has face-centred cubic structure with edge length equal to 361 pm. The apparent radius of atom 'A' is :

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 .

Iron (Il) oxide crystallise in cubic structure with unit cell edge of 5.0Å If the density of the oxide is 3.8 g cm-3 . Calculate the no. of Fe^2+ and O_2- present in each unit cell. [atomic mass of Fe=56, O=16]