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The density of crystalline CsCl is 3.988...

The density of crystalline `CsCl` is `3.988 g//cm^(3)`. The volume effectively occupied by a single `CsCl` ion pairs in the crystals is :(Given `CsCl` has mol. Mass `168.4`)

A

`7.014xx10^(-3) cm^3`

B

`7.014xx10^(-23) cm^3`

C

`1.014xx10^(-3) cm^3`

D

`1.542xx10^(-5) cm^3`

Text Solution

Verified by Experts

The correct Answer is:
B
For bcc structure of ionic compounds like CsCl, Z=1
`d=(ZxxM)/(N_Axxa^3)`
`a^3=(ZxxM)/(N_Axxd)`
`=(1xx168.4)/(3.988xx6.023xx10^23)=7.014xx10^(-23) cm^3`
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