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An element with molar mass 2.7 x 10-2kg mol-1 forms a cubic unit cell ...

An element with molar mass 2.7 x 10-2kg | Class 12 Chemistry Chapter The Solid State, The Solid State NCERT Solutions

Question:

An element with molar mass 2.7 x 10^-2kg mol^-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7 x 10³ kg m^-3, what is the nature of the cubic unit cell?

Answer:

It is given that density of the element, d = 2.7 ×10³ kg m^-3

Molar mass, M = 2.7 ×10^-2 kg mol^-1

Edge length, a= 405 pm = 405 ×10^-12 m = 4.05 ×10^-10m

It is known that, Avogadro's number, N_A= 6.022 ×10²³ mol^-1

Applying the relation, This implies that four atoms of the element are present per unit cell. Hence, the unit cell is face-centred cubic (fcc) or cubic close-packed (ccp).

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Welcome to the NCERT Solutions for Class 12 Chemistry - Chapter . This page offers a step-by-step solution to the specific question from Excercise 1 , Question 18: An element with molar mass 2.7 x 10-2kg mol-1 forms a cubic unit cell with edge length 405 pm. If it....

An element with molar mass 2.7 x 10-2kg | Class 12 Chemistry Chapter The Solid State, The Solid State NCERT Solutions

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