An element (atomic mass ) having BCC structure has a unit cell edge length of . Calculate its densit — Solid State Chemistry Question
Question
An element (atomic mass $100 \text{ g/mol}$) having BCC structure has a unit cell edge length of $400 \text{ pm}$. Calculate its density ($N_A = 6.02 \times 10^{23} \text{ mol}^{-1}$).
Answer: B
💡 Solution & Explanation
For BCC, $Z=2$. Convert $a=400\text{ pm}=4\times10^{-8}\text{ cm}$. Density is $\rho=\frac{ZM}{N_Aa^3}=\frac{2\times100}{6.02\times10^{23}\times(4\times10^{-8})^3}\approx5.19\text{ g/cm}^3$.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes