Question

a compound has BCC unit cell with edge length 10A°, if density is 2 gram per centimetre cube then molar mass of the compound is

Answer 1

i hope i am right if there's a problem with decimal u can adjust it thank you
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Answer 2

Given:

Density = 2

Z = 2 (As BCC unit cell)

To find:

Molar mass of the compound = ?

Formula to be used:

Density of unit cell = $\frac{Z\times M}{a^3\times N_a}$'

Where,

Z = No. of atoms

M = Mass

a= Bond length

Na= Avogadro constant

Calculation:

As 1 A° = 1×1$0^{-8}$ cm, ∴ 10A° = 1.0×$10^{-7}$

Substituting the values in the formula, it gives

M = $\frac{D\times a^3\times N_A}{Z}$

M = $\frac{2\times (1.0\times10^{-7})^3\times6.023\times10^{23}}{2}$

M = $1.0\times10^{-21}\times 6.023\times10^{23}$

M = $6.023\times10^2$

Conclusion:

The molar mass of the compound with BCC unit cell with edge length 10A°,and density 2 gram per centimeter cube is $6.023\times10^2$gm/mol.  

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