Question

A metal crystallizes in the HCP structure. It has a density of
12.87 g/cm3 and a lattice constant of

a = 0.564 nm. The height of the unit cell can be found from the
following relationship, c = 1.633a.

What is the atomic mass of this element?

Answer #1

The formula we are using here is given as:

d = (n * M) / (V * NA)

a is the lattice parameter = 0.564 nm = 0.564 * 10-7 cm

Given, c = 1.633 * a

Where, d is the density = 12.87 g/cm3

n is number of atoms in HCP = 6

M is atomic mass of the material = unknown

V is the volume = (3 * (3)1/2 * a2 * c) / 2

V = (3 * (3)1/2 * a2 * 1.633 * a) / 2

V = (3 * (3)1/2 * a3 * 1.633) / 2

V = 4.18 * (0.564 * 10-7 cm)3

V = 7.5 * 10-22 cm3

NA is the Avogadro number = 6.02 * 1023 atom/mol

Putting all values in the formula

d = (n * M) / (V * NA)

12.87 g/cm3 = (6 * M) / (7.5 * 10-22 cm3 * 6.02 * 1023 atom/mol)

12.87 g/cm3 = (6 * M) / (7.5 * 10-22 cm3 * 6.02 * 1023 atom/mol)

12.87 g/cm3 = (6 * M) / (451.5 cm3 .atom/mol)

(6 * M) = 12.87 g/cm3 * 451.5 cm3 .atom/mol

M = 968.4 g/mol

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.

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!

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).

A metal crystallizes in a face-centered cubic cell and had a
density of 11.9 g/cm3. If the radius of the metal atom is 138 pm,
what is the molar mass of the metal? What metal is it?

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....

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?

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 cubic close pack structure. The
edge of a unit cell is 408 pm and the density of the element is
19.27 g/cm^3. From the atomic mass of the element, the element is
:
(a) Ag (b) Au (c) W (d) P

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 19 minutes ago

asked 32 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 3 hours ago

asked 3 hours ago