Home
Class 12
CHEMISTRY
The density of a metal which crystallise...

The density of a metal which crystallises in bcc lattice with unit cell edge length 300 pm and molar mass `50 g "mol"^(-1)` will be:

A

`10gcm^(-3)`

B

`14.2 gcm^(-3)`

C

`6.15 gcm^(-3)`

D

`9.32gcm^(-3)`

Text Solution

Verified by Experts

The correct Answer is:
C
`rho =(2 xx 50)/(6.022 xx 10^23 xx (300)^3 xx (10^(-10))^3)`
` = 6.15 g//cm^3`
Promotional Banner

Topper's Solved these Questions

  • THE SOLID STATE

    ICSE|Exercise MULTIPLE CHOICE QUESTIONS (Formula based questions)|5 Videos

  • THE SOLID STATE

    ICSE|Exercise MULTIPLE CHOICE QUESTIONS (Fill in the blanks)|10 Videos

  • SURFACE CHEMISTRY

    ICSE|Exercise ISC EXAMINATION QUESTIONS |4 Videos

Similar Questions

Explore conceptually related problems

A metal crystallises in a bcc lattice ,its unit cell edge length in about 300 pm and its molar mass is about 50g mol^(-1) what would be the density of the metal (in g cm^(-3)) ?

Suppose the mass of a single Ag atoms is 'm' Ag metal crystallises in fcc lattice with unit cell edge length 'a' The density of Ag metal in terms of 'a' and 'm' is:

A metal crystallizes in bcc lattice. The percent fraction of edge length not covered by atom is

A metal crystallizes in a body-centred cubic lattice with the unit cell length 320 pm. The radius of the metal atom (in pm) will be

A substance has density of 2 kg dm^(-3) and it crystallizes to fcc lattice with edge length equal to 700 pm . The molar mass of the substance is _______ .

A compound AB crystallises in bcc lattice with the unit cell edge length of 380 pm . Calculate (i) The distance between oppositely charged Ions in the lattic. (ii)Radius of B^(−) if the radius of A^(+) is 190 pm.

A compound AB crystallises in the b.c.c lattice with unit cell edge length of 390 pm. Calculate (a) the distance between the oppsitely charged ions in the lattice. (b) the radius of A^(+) ion if radius of B^(-) ion is 175 pm.

An element exists in bcc lattice with a cell edge of 288 pm. Calculate its molar density is 7.2g//cm^(3)

Determine the type of cubic lattice to which a crystal belongs if the unit cell edge length is 290 pm and the density of crystal is 7.80g cm^(-3) . (Molar mass = 56 a.m.u.)

A compound XY crystallizes in BCC lattice with unit cell - edge length of 480 pm , if the radius of Y is 225 pm , then the radius of X is