Csbr crystallizes in a body centered cubic lattice

Asked by admin @ 27/08/2021 in Chemistry viewed by 305 People

CsBr crystallises in a BCC lattice. The unit cell of length is 436.6pm given that the atomic mass of Cs is 133 amu and of Br is 80 amu and the density of CsBr is

Answered by admin @ 27/08/2021

Answer:

The density of CsBr is $8.50 g/cm^3$ .

Explanation:

Number of atom in unit cell = Z = 4

Density of CsBr = ?

Edge length of cubic unit cell= a

Atomic mass of Pt(M) = 195.08 g/mol

Formula used :

$\rho=\frac{Z\times M}{N_{A}\times a^{3}}$

where,

$\rho$ = density

Z = number of atom in unit cell

M = Molar mass of compound

$(N_{A})$ = Avogadro's number

a = edge length of unit cell

We have:

M =133 g/mol + 80 g/mol = 213 g/mol

$a = 436.6 pm = 4.366\times 10^{-8} cm$

1 pm = $10^{-10} cm$

Z = 2

On substituting all the given values , we will get the value of 'a'.

$\rho=\frac{2\times 213 g/mol}{6.022\times 10^{23} mol^{-1}\times (4.366\times 10^{-8} cm)^{3}}$

$\rho = 8.50 g/cm^3$

The density of CsBr is $8.50 g/cm^3$ .

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