Iron has a body centred cubic unit cell with the dimension of 286.65 `p m`.The density of iron is 7.874 `g cm^-3`.Use this information to calculate avogadro's number. `(At mass of `Fe` = 55.845 `u`)`

Iron crystallizes in a body centred cubic structure. Calculate the radius of Fe if edge length of unit cell is 286 pm.

An element has a body centred cubic (bcc) 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?

A compound CuCl has face centred cubic structure. Its density is 3.4g cm^-3 .The length of unit cell is :

Calculate the number of moles in an iron bar dimension 10 cm xx 4 cm xx 2..5 cm density of iron being 7.85 gm/ cm^3

An element occurs in b c c structure with cell edge of 288 p m .Its density is 7.2 g cm^-3 . calculate the atomic mass of the element.

Copper crystallises with face centred cubic unit cell. If the radius of copper atom is 127.8 pm, calculate the density of copper metal. (Atomic mass of Cu= 63.55 u and Avogadro's number, N_(A)=6.02xx10^(23)"mol"^(-1) )

Determine the type of Cubic lattice to which the iron crystal belongs, if its density of 7.876 g//cm^3 and edge length of the cell is 286 pm. (At wt of Fe = 56)