Home
Class 12
CHEMISTRY
The body centered cubic cell of chronium...

The body centered cubic cell of chronium has an edge lenth of 0.288nm. Calculte the density of chromium `(g//cm^(3))` : `("Atomic mass": Cr=52.0)`

Text Solution

Verified by Experts

For bcc lacttice
`r = (sqrt3)/(4) = (sqrt3 xx 287)/(4) = 124.87 Å`
Density `(rho) = (Z_(eff) xx Mw)/(a^(3) xx N_(A))`
`(2 xx 51.99)/(287 xx 10^(-10))^(3) xx 6.023 xx 10^(23)`
`= 7.30 g cm^(-3)`
Promotional Banner

Topper's Solved these Questions

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.1 (Subjective)|12 Videos

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 1.1 (Objective)|19 Videos

  • SOLID STATE

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises (Archives ) Interger|1 Videos

  • REDUCTION AND OXIDATION REACTION OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise SUBJECTIVE TYPE|4 Videos

  • SOLUTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 2.3 (Objective)|9 Videos

Similar Questions

Explore conceptually related problems

The face centered cubic cell of platinum ha an edge length of 0.392nm. Calculate the density of platinum (g//cm^(3)) : ("Atomic mass": Pt=195)

Chromium metal crystallizes with a body-centred cubic lattice. The edge length of the unit cell is found to be 287 pm. Calculate the atomic radius. What would be the density of chromium in g cm^(-3) ? (atomic mass of Cr = 52.99)

A bcc element (atomic mass 65) has cell edge of 420 pm. Calculate its density in g cm^(-3) .

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

The elements crystallizes in a body centered cubic lattice and the edge of the unit cell is 0.351nm. The density is 0.533g//cm^(3) . What is the atomic mas?

An element crystallising in body centred cublic lattice has edge length of 500 pm. If the density is 4 g cm^(-3) , the atomic mass of the element ("in g mol"^(-1)) is (consider N_(A)=6xx10^(23))

An element crystallising in body centred cublic lattice has edge length of 500 pm. If the density is 4 g cm^(-3) , the atomic mass of the element ("in g mol"^(-1)) is (consider N_(A)=6xx10^(23))

A face-centred cubic element (atomic mass 60 ) has a cell edge of 400 pm. What is its density?

A face-centred cubic element (atomic mass 60 ) has a cell edge of 400 pm. What is its density?