Home
Class 12
CHEMISTRY
The atomic mass of a metal is 13.2484 g ...

The atomic mass of a metal is 13.2484 g `mol^(-1)`.It's crystal contains face centre cubic unit cell.Find the density of the metal in g `cm^(-3)` unit if the volume of the unit cell is `55times10^(-24)cm^(-3)` ? [`N_(A)=6.022times10^(23)`]

Promotional Banner

Similar Questions

Explore conceptually related problems

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.

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 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 ?

What is the volume of a face centred cubic unit cell, when its density is 2.0 g cm^(-3) and the molar mass of the substance is 60.23 g mol^(-1) ?

The density of a face centred cubic element (atomic mass = 40 ) is 4.25 gm cm^(-3) , calculate the edge length of the unit cell.

Zinc selenide, ZnSe, crystallizes in a face-centered cubic unit cell and has a density of 5.267 g/cc. Calculate the edge length of the unit cell.

Calcium crystallizes in a face centred cubic unit cell with a = 0.560 nm. The density of the metal if it contains 0.1% schottky defects would be:

An element (at. mass = 60) having face centred cubic unit cell has a density of 6.23g cm^(-3) . What is the edge length of the unit cell? (Avogadro's constant = 6.023 xx 10^(23) mol^(-1) )