QUESTION: Calculate the number of unit cells in 0.5 cm3 of iron solid sample if iron has an atomic diameter of 252 pm and crystallizes with a body-centered cubic structure.*Please use the pictures provided (the formula and some values that can be substituted) P:nAVCNAWhere: p density (g/cm³)n = no. of atoms/ unit cellA = atomic weight (g/mol)Importantconversion factors1 cm = 107 nm1 cm = 10¹⁰ pm1 cm = 10⁰ Å1 nm = 10 ÅVc = volume / unit cell (cm³/unit cell) = a³NA = Avogadro's number = 6.022x10²3 atoms/mol Coordination numberNumber of atoms perunit cellAPF (%)Relationship of r and aSC6152r =12αBCC8268r =√34aFCC12474r =√24a

Given the total volume of the solid iron, Vt = 0.5 cm3 Volume of one unit cell, Vc = a3 , where a…

Answered: Calculate the number of unit cells in…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter11: Liquids And Solids

Section: Chapter Questions

Problem 11.74QE

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QUESTION: Calculate the number of unit cells in 0.5 cm3 of iron solid sample if iron has an atomic diameter of 252 pm and crystallizes with a body-centered cubic structure.

*Please use the pictures provided (the formula and some values that can be substituted)

P:
nA
VCNA
Where: p density (g/cm³)
n = no. of atoms/ unit cell
A = atomic weight (g/mol)
Important
conversion factors
1 cm = 107 nm
1 cm = 10¹⁰ pm
1 cm = 10⁰ Å
1 nm = 10 Å
Vc = volume / unit cell (cm³/unit cell) = a³
NA = Avogadro's number = 6.022x10²3 atoms/mol

Coordination number
Number of atoms per
unit cell
APF (%)
Relationship of r and a
SC
6
1
52
r =
1
2
α
BCC
8
2
68
r =
√3
4
a
FCC
12
4
74
r =
√2
4
a

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