A molecule `A_(2)B (Mw = 166.4)` occupies triclinic lattice with `a = 5 Å, b = 8 Å`, and `c = 4 Å`,. If the density of `AB_(2)` is `5.2 g cm^(-3)`, the number of molecules present in one unit cell is

A molecule A_(2)B (Mw = 166.4) occupies triclinic lattice with a = 5 Å, b = 8 Å , and c = 4 Å ,. If the density of A_(2)B is 5.2 g cm^(-3) , the number of molecules present in one unit cell is

A molecule A_(2)B (Mw = 166.4) occupies triclinic lattice with a = 5 Å, b = 8 Å , and c = 4 Å ,. If the density of A_(2)B is 5.2 g cm^(-3) , the number of molecules present in one unit cell is

A molecule A_(2)B(MW = 166.4) occupies triclinic lattice with a = 5Å, b = 8Å, C = 4Å . If the density of A_(2)B is 5.2gm//cm^(3) the number of molecules present in one unit cell is?

A molecule A_(2)B (mol. wt 166.4) occupies triclinic lattice with a a=5Å, b=8Å and c = 4Å. If density of AB_(2) is 5.2 g cm^(-3) , calculate the number of molecules present in one unit cell

A molecule A_(2)B (molar mass=166.4) occupies triclinic lattice with a=5Å, b=8Å and c=4Å. If density of AB_(2) is 5.2 g cm^(-3) , the number of molecules present in one unit cell is:

A_(2)B molecules (" molar mass " = 259.8 g//"ml") crystallises in a hexagonal lattice as shown in figure .The lattic constants were a=5 Å and b=8 Å . If denstiy of crystal is 5 g//cm^(3) then how many molecules are contained in given unit cell ? (" Use" N_(A) = 6xx10^(23)) (a)6 (b)4 (c)3 (d)2

A metallic element has a cubic lattice. Each edge of the unit cell is 2 Å. The density of the metal is 2.5 g cm^(–3) . The number of unit cells in 200 g of the metal will be:

A_(2)B molecules (" molar mass " = 259.8 g//"ml") crystallises in a hexagonal lattice as shown in figure .The lattic constants were a=5 Å and b=8 Å . If denstiy of crystal is 5 g//cm^(3) then how many molecules are contained in given unit cell ? (" Use" N_(A) = 6xx10^(23))