Advertisements
Advertisements
Question
An element has a bee structure with unit cell edge length of 288 pm. How many unit cells and number of atoms are present in 200 g of the element?
Advertisements
Solution
For bcc unit cell, n = 2
Using formula (i),
Number of atoms in 200 g of element,
= `(200 g xx 2)/(14.44 g cm^-3 xx (2.88 xx 10^-8 cm)^3`
= 9.61 × 1024
Using formula (ii),
∴ Number of atoms in 200 g element is 9.61 × 1024
∵ Number of unit cells in 200 g element is 4.80 × 1024
APPEARS IN
RELATED QUESTIONS
An element with molar mass 27 g/mol forms a cubic unit cell with edge length of 405 p.m. If the density of the element is 2.7 g/cm3, what is the nature of the cubic unit cell?
Calculate the number of unit cells in 0.3 g of a species having density of 8.5 g/cm3 and unit cell edge length 3.25 × 10-8 cm.
Silver crystallises in fcc structure, if edge length of unit cell is 316.5 pm. What is the radius of silver atom?
An element crystallizes in fcc type of unit cell. The volume of one unit cell is 24.99 × 10-24 cm3 and density of the element 7.2 g cm-3, Calculate the number of unit cells in 36 g of pure sample of element?
What is the percentage of unoccupied space in fcc unit cell?
In bcc unit cell, the edge length (a) and radius of sphere (r) are related to each other by equation:
The percentage of unoccupied volume in simple cubic cell is ______.
A metal crystallises in bcc unit cell with edge length 'a'. What will be the volume of one atom?
An element crystallizes bcc type of unit cell, the density and edge length of unit cell is 4 g cm−3 and 500 pm respectively. What is the atomic mass of an element?
An element with density 2.8 g cm−3 forms fcc unit cell having edge length 4 × 10−8 cm. Calculate molar mass of the element.
Copper and silver have ____________ crystal structure.
Consider the following unit cell.
The number of particles (spheres) per unit cell is:
A metallic element has a cubic lattice with edge length of unit cell 2 Å. Calculate the number of unit cells in 200 g of the metal, if density of metal is 2.5 g cm-3?
What is the density of iron crystal which crystallizes in body-centred cubic structure with edge length 287 pm? (At. mass of Fe = 56 amu)
The coordination number of atoms in body-centred cubic structure (bcc) is ______.
A metal has an fcc lattice. The edge length of the unit cell is 404 pm. The density of the metal is 2.72 g cm−3. The molar mass of the metal is ______.
(NA Avogadro's constant = 6.02 × 1023 mol−1)
In face centred cubic unit cell, what is the volume occupied?
Identify unit cell from following having four particles in it
At room temperature, polonium Crystallises in a primitive cubic unit cell. If a = 3.36 Å. Calculate the theoretical density of polonium. [It's atomic weight is 209 g/mol.]
Silver crystallizes in the fcc structure. If the edge length of the unit cell is 400 pm, calculate the density of silver (Atomic mass of Ag = 108).
The correct sequence of the atomic layers in cubic close packing is ______.
The total number of different primitive unit cells is ______.
Which of the following metals exhibits minimum packing efficiency in its cubic system?
Calculate the molar mass of an element having density 2.8 g cm−3 and forms fcc unit cell.
[a3.NA = 38.5 cm3 mol−1]
