Question
Calculate the density of an element having molar mass 225\ g mol ^ -1 forming bcc structure [a^3 N_A = 75\ cm ^3 mol ^ -1 ]
MHT CET
Chemistry
Solid State
2026
MHT CET 2026 (20 April Shift 1)
MHT CET Chemistry Question (2026) — Solution
Options
- A. 6.0 g cm^ -3
- B. 2.81 g cm^ -3
- C. 9.24 g cm^ -3
- D. 11.36 g cm^ -3
Answer
A. 6.0 g cm^ -3
Step-by-step solution
For a body-centered cubic (bcc) structure, the number of atoms per unit cell is Z = 2. The formula for the density of a unit cell is given by: d = Z M a^3 N_A Substituting the given values Z = 2, M = 225\ g mol ^ -1 , and a^3 N_A = 75\ cm ^3 mol ^ -1 : d = 2 225 75 d = 450 75 = 6.0\ g cm ^ -3 Answer: 6.0 g cm^ -3
Related: Chemistry — Solid State · All PYQ Banks