MHT CET · Chemistry · Solid State

What is the mass of bcc type unit cell of sodium if mass of one atom of sodium is \(3 \cdot 819 \times 10^{-23} \mathrm{~g}\) ?

A \(7 \cdot 038 \times 10^{-23} \mathrm{~g}\)
B \(7 \cdot 638 \times 10^{-23} \mathrm{~g}\)
C \(3 \cdot 819 \times 10^{-23} \mathrm{~g}\)
D \(1.5276 \times 10^{-22} \mathrm{~g}\)

Verified Solution

Answer & Solution

Correct Answer

(B) \(7 \cdot 638 \times 10^{-23} \mathrm{~g}\)

Step-by-step Solution

Detailed explanation

No. of atoms per bcc type of unit cell, \(\mathrm{n}=2\)
Mass of bcc unit cell \(=\) Mass of two atoms
\(\therefore \text {Mass of bcc unit cell of } \mathrm{Na}\) \(=3.819 \times 10^{-23} \times 2\)
\(=7.638 \times 10^{-23} \mathrm{~g}\)

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.

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