[CsBr has CsCl type structure. Its density is 4.26g/ml. The side of unit cell is (Cs=133,Br=80)

The compound CuCl has Zns structure. Its edge length is 420 pm. What is the density of the unit cell ? (Atomic mass of CuCl=99)

The cubic unit cell of a metal (molar mass= 63.55 g "mol"^(-1) ) has an edge length of 362pm. Its density is 8.92gcm^(-3) . The type of unit cell is

A compound CuCl has face - centred cubic structure. Its density is 3.4g cm^(-3) . What is the length of unit cell ?

A compound CuCl has face - centred cubic structure. Its density is 3.4g cm^(-3) . What is the length of unit cell ?

An element crystallizes as body - centred cubic lattic. Its density is 7.12g cm^(-3 and the length of the side of the unit cell is 2.88Å . Calculate the number of atoms present is 288g of the element.

CsCl has cubic structure. Its density is 3.99 g cm^(-3) . What is the distance between Cs^(o+) and Cl^(Θ) ions? (Atomic mass of Cs = 133 )

The cubic unit cell of Al (molar mass 27 g "mol"^(-1) ) has an edge length of 405 pm. Its density is 2.7gcm^(-3) . The cubic unit cell is :

The density of CaF_(2) (flourtie structure ) is 3.18 g// cm^(3) . The length of the side of the unit cell is :

A solid AB has CsCl -type structure. The edge length of the unit cell is 404 pm. Calculate the distance of closest approach between A^(o+) and B^(Θ) ions.

Al (atomic mass =27) crystallises in a cubic system with edge length (a) equal to 4Å its density is 2.7 g//cm^(3) The type of the unit cell is: