Question

The density of solid Fe is 7.87 g/cm3. How many atoms are present per cubic centimeter of Fe? As a solid, Fe adopts a body-centered cubic unit cell. How many unit cells are present per cubic centimeter of Fe? What is the volume of a unit cell of this metal? What is the edge length of a unit cell of Fe?

Answer #1

Nickel crystallizes in a face-centered cubic lattice. If the
density of the metal is 8.908 g/cm3, what is the unit cell edge
length in pm?

1. Rubidium metal has a
body-centered cubic structure. The density of the metal is 1.532
g/cm3. Calculate the radius of the rubidium atom. Assume
that rubidium atoms are spheres. Then note that each corner sphere
of the unit cell touches the body-centered sphere.
2. Copper metal has a face-centered
cubic structure. The density of the metal is 8.93 g/cm3.
Calculate the radius of the copper atom. Assume that copper atoms
are spheres. Then note that the spheres on any face...

An unknown metal is found to have a density of 7.8748 g/cm3 and
to crystallize in a body-centered cubic lattice. The edge of the
unit cell is found to be 0.28864 nm . Calculate the atomic mass of
the metal.

Copper crystallizes with a face-centered cubic lattice and has a
density of 8.93 g/cm3.
a.) Calculate the mass of one unit cell of copper (in grams) b.)
Calculate the volume of the copper unit cell (in cm3). c.)
Calculate the edge length of the unit cell (in cm). d.) Calculate
the radius of a copper atom (in pm).

An unknown metal is found to have a density of 7.1800 g/cm3 and
to crystallize in a body-centered cubic lattice. The edge of the
unit cell is found to be 0.28864 nm .
Calculate the atomic mass of the metal.
please show all formulas and units!

Iron (Fe) crystallizes in a body-centered cubic structure with
a lattice constant of 0.287 nm:
Use drawing to show how the iron atoms are packed in the unit
cell. How many iron atoms are contained in each unit
cell?
Use drawings to show how the iron atoms are arranged on the
(100) and (110)
planes.
Determine the density of iron (g/cm3) by dividing
the total mass of iron atoms in the unit cell by the volume of the
unit cell....

Iron (Fe) crystallizes in a body-centered cubic structure with a
lattice constant of 0.287 nm:
a. Use drawing to show how the iron atoms are packed in the unit
cell. How many iron atoms are contained in each unit
cell?
b. Use drawings to show how the iron atoms are arranged on the
(100) and (110)
planes.
c. Determine diameter of iron atom
d. Determine the density of iron (g/cm3) by dividing
the total mass of iron atoms in...

Iron (Fe) crystallizes in a body-centered cubic structure with a
lattice constant of 0.287 nm:
a. Use drawing to show how the iron atoms are packed in the unit
cell. How many iron atoms are contained in each unit
cell?
b. Use drawings to show how the iron atoms are arranged on the
(100) and (110)
planes.
c. Determine diameter of iron atom
d. Determine the density of iron (g/cm3) by dividing
the total mass of iron atoms in...

Iridium packs in a face centered cubic structure with a density
of 22.43 g/cm3 . Calculate the following: (1) Volume of unit cell
in pm3 . (2) cell length (3) radius of iridium.

The substance calcium is found to crystallize
in a cubic lattice, with an edge length of 556.0
pm. If the density of solid calcium is
1.549 g/cm3, how many
Ca atoms are there per unit cell?
Your answer should be an integer:______ atoms

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