Fe has a BCC structure and an atomic radius of 0.126 nm. The atomic mass of Fe is 55.85 g/mol & Avogadro's No. is 6.023 x 1023. Calculate the density of Fe.
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Answer:
Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight of 55.85...
Question:
Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight of 55.85 g/mol. Compute and compare its theoretical density with the commonly used value (experimentally obtained) of {eq}7.87 g/cm^3{/eq}.
Density of Cubic Crystal
The unit cell density can be calculated by taking the ratio of its mass to the volume. The density of the different types of cubic lattices depend upon the atoms which are present inside the unit cell.
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Given Data:
The edge length of metal is 0.124 nm.
The experimental density is {eq}7.87\;{\rm{g/c}}{{\rm{m}}^{\rm{3}}} {/eq}
The molar mass of iron...
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Crystal Structures and the Unit Cell
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Chapter 6 / Lesson 4
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This crystallography lesson explores the structure and properties of crystals. You'll learn about the parts of a crystal structure, types of crystals and patterns created by unit cells.