04 Chap 01 Solid State | ठोस अवस्था | Unit Cell Density and Numercals | Vikram HAP Chemistry

A crystalline solid AB adopts sodium chloride type structure with edge length of the unit cell as 745 pm and formula mass of 74.5 g The density of the crystalline compound is

(a) An element has atomic mass 93 g mol^(_1) and density 11.5 g cm^(-3) . If the edge length of its unit cell is 300 pm, identify the type of unit cell. (b) Write any two differences between amorphous solids and crystalline solids.

X=5Å Y=8Å Molar mass of solid ="259.8 g mol"^(-1) A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is 5g/ml. How many molecules are their in the given unit cell? ("Avagadro's number "=6.023xx10^(23))

Methane crystallises in a cubic unit cell with a = 0.598 nm. Calculate the theoretical density of methane assuming Z = 1, 2 and 4. If the density of liquid methane is 0.466"g cm"^(-3) and assume that density of solid is the same as that of the liquid at a given temperature, predict which type of unit cell result?