TS EAMCET · Chemistry · Solid State

Iron crystalizes in $FCC$ with an edge length of $400 pm$ . If it contains $0.1 %$ Schottky defects, calculate its approximate density [ $AW$ of $Fe = 56 g / mol$ ]

A $5.8 g / {cm}^{3}$
B $1.5 g / {cm}^{3}$
C $2.9 g / {cm}^{3}$
D $8.5 g / {cm}^{3}$

Verified Solution

Answer & Solution

Correct Answer

(A) $5.8 g / {cm}^{3}$

Step-by-step Solution

Detailed explanation

In a solid with Schottky defect atoms are missing from their position. Thus, the effective number of formula units per unit cell will decrease. so, density will also decrease. For FCC lattice with 0.1% Schottky defect, the effective atoms per unit cell,…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

Same subject

List - 1 (Chemical)	List-2 (Type)
A	Bithionol	I	Artificial sweetener
B	Saccharin	II	Antifertility drug
C	Sodium benzoate	III	Antiseptic
D	Norethindrone	IV	Food preservative

Explore more questions on app

From TS EAMCET

Explore more questions on app

Iron crystalizes in FCC with an edge length of 400pm. If it contains 0.1% Schottky defects, calculate its approximate density [AW of Fe=56 g/mol]

Step-by-step Solution

Iron crystalizes in $FCC$ with an edge length of $400 pm$ . If it contains $0.1 %$ Schottky defects, calculate its approximate density [ $AW$ of $Fe = 56 g / mol$ ]