Question

- 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/cm
^{3)}by dividing the total mass of iron atoms in the unit cell by the volume of the unit cell. The atomic mass of iron is 55.845 amu and the Avogadro’s number is 6.02x10^{23}

Answer #1

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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...

An element crystallizes in a body-centered cubic lattice. The
edge of the unit cell is 3.37 Å in length, and the density of the
crystal is 7.88 g/cm3 .
Calculate the atomic weight of the element.
Express the atomic weight in grams per mole to three significant
digits.

Chromium metal crystallizes as a body-centered cubic lattice. If
the atomic radius of Cr is 1.25 angstroms, what is the density of
Cr metal in g/cm3?

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?

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).

If the atomic radius of potassium is 227 pm and potassium
crystallizes in a body-centered cubic shape, What is the volume in
cm3 of a unit cell of potassium to 3 sig figs

A certain element crystallizes in a face-centered cubic lattice.
The density of the crystal is 22.67 g·cm–3, and the edge of the
unit cell is 383.3 pm. Calculate the atomic mass of the element.
(a) 192 g·mol–1 (b) 40 g·mol–1 (c) 183 g·mol–1 (d) 70 g·mol–1 (e)
None of the above

Chromium crystallizes in a body-centered cubic unit cell with an
edge length of 2.885 Å.
(a) What is the atomic radius (in Å) of chromium in this
structure?
____ Å
(b) Calculate the density (in g/cm3) of chromium.
____ g/cm3

They metal crystallizes in a face center cubic lattice. The radius
of the atom is 196 PM and the density of the element is 1.55 g/cm3.
How many atoms are there per unit cell?

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