Question

The density of solid Fe is 7.87 g/cm3. How many atoms are present per cubic centimeter...

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?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
If the density of solid chromium is 7.15 g/cm3, what is the packing efficiency of Cr...
If the density of solid chromium is 7.15 g/cm3, what is the packing efficiency of Cr if it adopts a body-centered cubic unit cell? The molar mass of Cr is 51.996 g/mol.
Nickel crystallizes in a face-centered cubic lattice. If the density of the metal is 8.908 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?
1. Rubidium metal has a body-centered cubic structure. The density of the metal is 1.532 g/cm3....
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...
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...
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).
Iron (Fe) crystallizes in a body-centered cubic structure with a lattice constant of 0.287 nm: Use...
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....
An unknown metal is found to have a density of 7.1800 g/cm3 and to crystallize in...
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: a....
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....
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...
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.