An element (atomic mass 100 g / mol ) having BCC structure has unit cell edge 400 pm. The density of element is (No. of atom in BCC ( Z )=2 ).

Question

An element (atomic mass 100 g / mol ) having BCC structure has unit cell edge 400 pm. The density of element is (No. of atom in BCC ( Z )=2 ). (A) 10.376 g/cm3 (B) 5.1888 g/cm3 (C) 7.289 g/cm3 (D) 2.144 g/cm3

Tardigrade Admin · Accepted Answer

No. of atoms per unit cell in b.c.c. lattice (n) = 2 Density, d = (n × M/a3 × NA) = (2× 100/(4× 10-8 cm)3 × 6.02 × 1023) = (200/38.528) = 5.19 g/cm3.

Q. An element (atomic mass $100 g / m o l$ ) having $BCC$ structure has unit cell edge $400 p m$ . The density of element is (No. of atom in $BCC (Z) = 2$ ).

$10.376 g / c m^{3}$

$5.1888 g / c m^{3}$

$7.289 g / c m^{3}$

$2.144 g / c m^{3}$

No. of atoms per unit cell in $b . c . c .$ lattice $(n) = 2$

Density, $d = \frac{n \times M}{a ^{3} \times N _{A}}$

$= \frac{2 \times 100}{( 4 \times 1 0 ^{- 8} c m ) ^{3} \times 6.02 \times 1 0 ^{23}}$

$= \frac{200}{38.528}$

$= 5.19 g / c m^{3}$ .

Q. An element (atomic mass 100g/mol ) having BCC structure has unit cell edge 400pm. The density of element is (No. of atom in BCC(Z)=2 ).

10.376g/cm3

5.1888g/cm3

7.289g/cm3

2.144g/cm3