Question

an element with molar mass 2.7×10^-2 kg mol^-1 form a cubic unit cell with edge length 405 pm if its density is 2.7 * 10^23 kgm^-3 what is the nature of cubic unit cell

Answer 1

Answer:

Hii

An element with molar mass 2.7×10-2 kg mol-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7×103 kg m-3 , what is the nature of the cubic unit cell ? Thus, there are 4 atoms of the element present per unit cell. Hence, the cubic unit cell must be face centred or cubic close packed (ccp).

Answer 2

Heya user.......❤

Question :an element with molar mass 2.7×10^-2 kg mol^-1 form a cubic unit cell with edge length 405 pm if its density is 2.7 * 10^3 kgm^-3 what is the nature of cubic unit cell?

Solution :

Given, density = 2.7*10^3 kgm^-3

Molar mass = 2.7*10^-2kgmol^-1

Edge length = 405 pm = 4.05*10^-10m

As we know, Avogadro's number, NA = 6.02*10^23 mol^-1

Hence, applying the relation,

d = (d a^3 NA) /M

= ( 2.7*10^3) × ( 4.05*10^-10)^3 × ( 6.02*10^23) / (2.7*10^-2)

= 4.004

= 4

It implies that 4 atoms of the elements are present per unit cell.So, the unit is faced -centred cubic face ( FCC) or cubic closed packed (ccp).

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