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The Solid State

Long Answer Type

151. An element occurs in BCC structure with cell edge of 300 pm. The density of the element is 5.2 g cm^–3. How many atoms of the element does 200 g of the element contain?

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Short Answer Type

152. Iron (II) oxide has a cubic structure and each unit cell has side 5A. If the density of the oxide is 4 g cm^–3, calculate the number of Fe²⁺ and O^2– ions present in each unit cell. (Molar mass of FeO = 72 g mol^–1, N_A = 6.02 x 10²³ mol^–1).

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153. A metallic element exists as a cubic lattice. Each edge of the unit cell is 2.88 A°. The density of the metal is 7.20 g cm^–3. How many unit cells will be there in 100 g of the metal?

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154. The unit cell of an element of atomic mass 96, and density 10.3 g cm^–3 is a cube with edge length of 314 pm. Find the structure of crystal lattice (simple cubic, F.C.C. or B.C.C.) Avogadro’s constant. N_A = 6.023 x 10²³ mol^–1?

solution:
we have given

Density of element, $ρ = 10.3 g {cm}^{- 3}$
Cell edge a= 314pm or 3.14 x 10^-10 cm

$N_{A} = 6.023 \times 10^{23} {mol}^{- 1}$

Atomic mass $= 96 g {mol}^{- 1}$

$P = \frac{Z \times M}{a^{3} \times N_{A}} Z = \frac{P \times a^{3} \times N_{A}}{M}$

$= \frac{10 . g {cm}^{- 3} \times (3.14)^{3} \times 10^{- 30} {cm}^{3} \times 6.023 \times 10^{23} {mol}^{- 1}}{96 g {mol}^{- 1}} = 2$

The structure of the crystal lattice is B.C.C.

2325 Views

Long Answer Type

155. An element a crystallises in fcc structure. 200 g of this element has 4.12 x 10²⁴atoms. The density of A is 7.2 g cm^-3. Calculate the edge length of the unit cell?

1979 Views

Short Answer Type

156. An element crystallises in BCC structure. The edge length of its unit cell is 288 pm. If the density of crystal is 7.2 g cm^–3, what is the atomic mass of the element?

1664 Views

Long Answer Type

157. Caesium chloride crystallises as a body centred cubic lattice and has a density of 4.0 g cm^–3. Calculate the length of the edge of the unit cell of caesium chloride crystal.
[Molar Mass of CsCl = 168.5 g mol^–1, N_A = 6.02 x 10²³ mol^–1]

564 Views

Short Answer Type

158. The density of chromium is 7.2 g cm^–3. If the unit cell is cubic with edge length of 289 pm, determine the type of the unit cell (Atomic mass of Cr = 52 amu).

1682 Views

Long Answer Type

159. Iron (II) oxide has a cubic structure and each of the unit cell is 5.0 A°. If density of the oxide is 4.0 g cm^-3, calculate the number of Fe²⁺and O^2– ions present in each unit cell.

341 Views