AP EAMCET · Chemistry · Solid State
An element has a body centered cubic structure with a unit cell edge length of \(400 \mathrm{pm}\). Atomic mass of an element is \(24 \mathrm{~g} \mathrm{~mol}^{-1}\). What is the density of the element?
\[
\left(\mathrm{N}_{\mathrm{A}}=6 \times 10^{23} \mathrm{~mol}^{-1}\right)
\]
- A \(2.50 \mathrm{~g} \mathrm{~cm}^{-3}\)
- B \(1.80 \mathrm{~g} \mathrm{~cm}^{-3}\)
- C \(3.60 \mathrm{~g} \mathrm{~cm}^{-3}\)
- D \(1.25 \mathrm{~g} \mathrm{~cm}^{-3}\)
Answer & Solution
Correct Answer
(D) \(1.25 \mathrm{~g} \mathrm{~cm}^{-3}\)
Step-by-step Solution
Detailed explanation
Given, Body centered cubic (bcc) \(Z=2\) Edge length \((a)=400 \mathrm{pm}=400 \times 10^{-10}\) \(M(\) Atomic mass \()=24 \mathrm{~g} \mathrm{~mol}^{-1}\) \(\because \quad\) Density \((d)=\frac{Z \times M}{a^3 \times N_A}\)…
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