Derive the relationship between density of substance, its molar mass and the unit cell edge length. Explain how you will calculate the number of particles, and number of unit cells in x g of metal.

The density of Cr atoms is 7.02g//cm . If the unit cell has edge length 289p m . Calculate the number of chromium atoms per unit cell. (at masss of Cr=52) .

An element 'x' (Atomic mass = 40 g mol^(-1) ) having f.c.c. structure has unit cell edge length of 400 pm. Calculate the density of 'x' and the number of unit cells in 4 g of 'x'

An element A (Atomic weight =100 ) having b.c.c. structures has unit cell edge length 400 pm. Calculate the density of A. number of unit cells and number of atoms in 10 g of A.

A substance crystallizes in fcc structure. The unit cell edge length is 367.8pm. Calculate the molar mass of the substance if its density is 21.5 g//cm^3

If the unit cell edge length of NaCl crystal is 600 pm, then the density will be

An element (density 7.2 g cm^(-3)) crystallizes in a body centred cubic structure having its unit cell edge length 2.88 Å . Calculate the number of atoms present in 156 g of the element.

Density of a unit cell is same as the density of the substance. If the density of the substance is known, number of atoms or dimensions of the unit cell can be calculated . The density of the unit cell is related to its mass(M), no. of atoms per unit cell (Z), edge length (a in cm) and Avogadro number N_A as : rho = (Z xx M)/(a^3 xx N_A) A metal X (at. mass = 60) has a body centred cubic crystal structure. The density of the metal is 4.2 g cm^(-3) . The volume of unit cell is

Density of a unit cell is same as the density of the substance. If the density of the substance is known, number of atoms or dimensions of the unit cell can be calculated . The density of the unit cell is related to its mass(M), no. of atoms per unit cell (Z), edge length (a in cm) and Avogadro number N_A as : rho = (Z xx M)/(a^3 xx N_A) The number of atoms present in 100 g of a bcc crystal (density = 12.5 g cm^(-3)) having cell edge 200 pm is

Density of a unit cell is same as the density of the substance. If the density of the substance is known, number of atoms or dimensions of the unit cell can be calculated . The density of the unit cell is related to its mass(M), no. of atoms per unit cell (Z), edge length (a in cm) and Avogadro number N_A as : rho = (Z xx M)/(a^3 xx N_A) An element crystallizes in a structure having a fcc unit-cell an edge 100 pm. If 24 g of the element contains 24 xx 10^(23) atoms, the density is

A metallic element crystallizes in simple cubic lattice. Each edge length of the unit cell is 3 Å.The density of the element is 8g//c c . Number of unit cells in 108 g of metal is