Question

6. Calculate the density of the bcc lattice if its edge length
is 409 pm. Its molar mass is 216.3 g mol-1 and
Avogadro number is 6.02 x 1023 mol-1.​

Answer 1

Answer:

12th

Chemistry

The Solid State

Packing Efficiency and Calculations Involving Unit Cell Dimensions

Metal has an fcc lattice. T...

CHEMISTRY

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 (in g mol

−1

) of the metal is:

[Avogadro's constant =N

A

=6.02×10

23

mol

−1

]

MEDIUM

Share

Study later

VIDEO EXPLANATION

ANSWER

The formula for the density of the metal is as given below:

d=

V×N

A

Z×M

Substituting values in the above expression, we get

2.72=

(4.04×10

−8

)

3

×6.02×10

23

4×M

M=

4

2.72×(4.04)

3

×6.02×10

−1

=27 g/mol

Hence, the molar mass of the metal is 27 g/mol.

Hence, the correct option is C

Explanation:

please please follow me and mark My is the best