Calculate the density of an element having molar mass $225 \text{ g mol}^{-1}$ forming a $bcc$ structure. Given: $[a^3 \times N_A = 75 \text{ cm}^3 \text{ mol}^{-1}]$ (in $\text{ g cm}^{-3}$)
- A$6.0$
- B$2.81$
- C$9.24$
- D$11.36$
Explore More
Similar Questions
Find the radius of a metal atom in a $bcc$ unit cell having an edge length of $450 \ pm$. (in $pm$)
Silver forms a $CCP$ structure and its density is $10.5 \ g/cm^3$. What is the edge length of the unit cell? (Molar mass of silver is $107.9 \ g/mol$)
Calculate the volume of $fcc$ unit cell if the radius of a particle in it is $106.05 \ pm$.
If an element having atomic number $96$ crystallises in a cubic lattice with a density of $10.3 \ g \ cm^{-3}$ and an edge length of $314 \ pm$, then the structure of the solid is:
What is the length of the body diagonal in a $bcc$ structure?
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo