Calculation of Density of Unit Cell

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Calculation of Density of Unit Cell: Overview

This topic covers concepts, such as, Density of a Cubic Crystal System etc.

Important Questions on Calculation of Density of Unit Cell

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Calcium crystallizes in a face centred cubic unit cell with a =0.560nm.  The density of the metal if it contains 0.1% schottky defects would be:

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Copper crystallises in a face-centred cubic lattice and has a density of  8.930gcm3 at 393 K. The radius of a copper atom is:
[Atomic mass ofCu=63.55u,NA=6.02×1023mol1]

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Iron has a body-centered cubic unit cell of cell edge 286.65 pm. The density of iron is 7.87 g cm-3. The Avogadro number is

(Atomic mass of iron =56 gmol1)

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X-rays diffraction studies show that copper crystallizes in an FCC unit cell with cell edge of  3.6885×108cm. In a separate experiment, copper is determined to have a density of   8 .92g/cm 3 , the atomic mass of copper would be:

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In face-centred cubic (FCC) and body centred cubic (BCC), whose unit cell lengths are 3.5 and 3.0 Å respectively, a metal crystallises into two cubic phases. What is the ratio of densities of FCC and BCC?

the ratio of densities of fcc and bcc. the solid state jee jee mains Share It On Read more on Sarthaks.com - https://www.sarthaks.com/299362/metal-crystallizes-into-two-cubic-phases-face-centred-cubic-fcc-and-body-centred-cubic-bcc
ratio of densities of fcc and bcc. Read more on Sarthaks.com - https://www.sarthaks.com/299362/metal-crystallizes-into-two-cubic-phases-face-centred-cubic-fcc-and-body-centred-cubic-bcc

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A unit cell of sodium chloride has four formula units with an edge length of the unit cell 0.564 nm. What is the density of sodium chloride?

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A compound AB has rock salt type structure. The formula weight of AB is 6.023 Y amu, and the closest AB distance is Y 1 3 nm, where Y is an arbitrary number. The density of lattice is

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The density of mercury is 13.6 g ml-1. The approximate diameter of an atom of mercury assuming that each atom is occupying a cube of edge length equal to the diameter of the mercury atom is

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Copper crystallizes in an FCC unit cell with cell edge of  3.608×108cm. The density of copper is  8.92 g/cm3, Calculate the atomic mass of copper.

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Ice crystallises in a hexagonal lattice. At the low temperature at which the structure was determined, the lattice constants were a=4.53 Å and c=7.41 Å. How many H2O molecules are contained in a unit cell? The density of ice is 0.92 g/cc at 0 °C. A unit cell of H2O is shown below:

 Question Image

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Iron exhibits BCC-structure at room temperature. Above 500°C, it transforms to FCC-structure. Find the ratio of the density of iron at room temperature to that at 500°C. (Assume the atomic radii and the molar mass of iron remain constant even with variation in temperature)

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If each edge of a cubic unit cell of an element having atomic mass 120 and density 6.25 g.cc-1 measures 400 pm, then the crystal lattice is

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Al (atomic weight 26.98) crystallizes in the cubic system with a = 4.05 Å. Its density is 2.7 g per cm3. Determine the cell type. Calculate the radius of Al atom.

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Zinc selenide(ZnSe) crystallizes in a face-centred cubic unit cell and has a density of 5.267 g/cc. Calculate the edge length of the unit cell.

Give the answer as the nearest integer.

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An unknown metal is found to have a density of 10.2 g/cc at 25°C. It is found to crystallize in a body-centered cubic lattice with a unit cell edge length of 3.147 Å. Calculate the molar mass of the metal in grams.

Give your answer as the nearest integer.

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Metallic rhodium crystallizes in a face-centered cubic lattice with a unit-cell edge length of 3.803 Å Calculate the molar volume (in cm3) of rhodium including the empty spaces. (Give answer after rounding off to the nearest integer value.)

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The unit cell of copper corresponds to a face centered cube of edge length 3.596 Å with one copper atom at each lattice point. The calculated density of copper in kg/m3 is _________. [Molar mass of Cu=63.54 g; Avogadro's number =6.022×1023] (Round off answer to nearest integer value).

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An element with molar mass 2.7×10-2 kg mol-1 forms a cubic unit cell with edge length 405 pm. If its density is 2.7×103 kg m-3, the radius of the element is approximately ×10-12 m (to the nearest integer).

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An element crystallizes in a structure having fcc unit cell of an edge 200 pm. Calculate the density in g/cc, if 200 g of this element contains 5×1024  atoms.

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The density of iron crystal is 8.54 g cm3. If the edge length of unit cell is 2.8 Å and atomic mass is 56 g mol1, find the number of atoms in the unit cell. (Given: Avogadro’s number = 6.022 × 1023, 1 Å = 1 × 108 cm)