A solid having density of 9 × 103 kg m -3 forms face centred cubic crystals of edge length 200 √2 pm. What is the molar mass of the solid? [. Avogadro constant .≃ 6 × 1023 mol -1, π ≃ 3]

Question

A solid having density of 9 × 103 kg m -3 forms face centred cubic crystals of edge length 200 √2 pm. What is the molar mass of the solid? [. Avogadro constant .≃ 6 × 1023 mol -1, π ≃ 3] (A) 0.0216 kg mol -1 (B) 0.0305 kg mol -1 (C) 0.4320 kg mol-1 (D) 0.0432 kg mol-1

Tardigrade Admin · Accepted Answer

Formula for density, Density, d =( Z × M / a 3 × N A ) where, d = density of the unit cell M = Molar mass of the molecule a3= volume of the unit cell N A = Avogadro number Here, for FCC unit cell, Z = 4 Subsituting the values we get, 9 × 103=(4 × M /(200 √2 × 10-12)3 × 6.0 × 1023) ⇒ M =0.0305 kg .mol -1

Q. A solid having density of $9 \times 1 0^{3} k g m^{- 3}$ forms face centred cubic crystals of edge length $2002 p m$ . What is the molar mass of the solid?
$[$ Avogadro constant $≃ 6 \times 1 0^{23} m o l^{- 1}, π ≃ 3]$

$0.0216 k g m o l^{- 1}$

$0.0305 k g m o l^{- 1}$

$0.4320 k g m o l^{- 1}$

$0.0432 k g m o l^{- 1}$

Q. A solid having density of 9×103kgm−3 forms face centred cubic crystals of edge length 2002​pm. What is the molar mass of the solid? [ Avogadro constant ≃6×1023mol−1,π≃3]

0.0216kgmol−1

0.0305kgmol−1

0.4320kgmol−1

0.0432kgmol−1

Formula for density, Density, d=a3×NA​Z×M​ where, d= density of the unit cell M= Molar mass of the molecule a3= volume of the unit cell NA​= Avogadro number Here, for FCC unit cell, Z=4 Subsituting the values we get, 9×103=(2002​×10−12)3×6.0×10234×M​ ⇒M=0.0305kg.mol−1

Q. A solid having density of $9 \times 1 0^{3} k g m^{- 3}$ forms face centred cubic crystals of edge length $2002 p m$ . What is the molar mass of the solid?
$[$ Avogadro constant $≃ 6 \times 1 0^{23} m o l^{- 1}, π ≃ 3]$

$0.0216 k g m o l^{- 1}$

$0.0305 k g m o l^{- 1}$

$0.4320 k g m o l^{- 1}$

$0.0432 k g m o l^{- 1}$