Question

Gold, which has a density of 19.32 g/cm^{3}, is the most
ductile metal and can be pressed into a thin leaf or drawn out into
a long fiber.

**(a)** If a sample of gold with a mass of 8.953 g,
is pressed into a leaf of 2.403 μm thickness, what is the area of
the leaf?

**(b)** If, instead, the gold is drawn out into a
cylindrical fiber of radius 2.100 μm, what is the length of the
fiber?

Answer #1

Gold, which has a density of 19.32 g/cm3, is the most ductile
metal and can be pressed into a thin leaf or drawn out into a long
fiber. (a) If a sample of gold with a mass of 1.891 g, is pressed
into a leaf of 5.173 μm thickness, what is the area of the leaf?
(b) If, instead, the gold is drawn out into a cylindrical fiber of
radius 2.900 μm, what is the length of the fiber?

Gold, which has a density of 19.32 g/cm3, is the most
ductile metal and can be pressed into a thin leaf or drawn out into
a long fiber. (a) If a sample of gold with a mass
of 3.245 g, is pressed into a leaf of 3.989 ?m thickness, what is
the area of the leaf? (b) If, instead, the gold is
drawn out into a cylindrical fiber of radius 2.700 ?m, what is the
length of the fiber?

Gold, which has a density of 19.32 g/cm^3, is the most ductile
metal and can be pressed into a thin leaf or drawn out into a long
fiber. If a sample of gold with a mass of 5.58 g is drawn out into
a cylindrical fiber of radius 1.87 μm, what is the length (in km)
of the fiber? Express your answer to 3 significant figures.

Gold has a density of 19.3 g/cm3, and quartz has a
density of 2.65 g/cm3. A sample of quartz contains gold.
If the quartz sample has a mass of 10 g and a volume of 3
cm3, what is the mass in grams of gold in the quartz
sample?

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?

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...

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?

The very dense metal iridium has a face centered cubic structure
and density of 22.56 g/cm3. use this information to calculate the
radius of an iridium atom.

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).

Consider a hypothetical metal that has a simple cubic structure,
a density of 9.62 g/cm3, and an atomic weight of 90.5
g/mol. If, at the melting temperature, one out of every
104 atom sites is a vacancy, determine the number of
vacancies in one cubic meter of this material. Assume that the
energy for the vacancy formation is 96,000 J/mol.
Answer should be in units of vacancies/m^3

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