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The degree of dissociation is 0.4 at 400...

The degree of dissociation is 0.4 at 400 K and a I atm for the gaseous reaction: `PCI_(5(g)) hArr PCl_(3(g)) +Cl_(2(g))` : assuming ideal behaviour of gases, calculate the density of cquilibrium mixture at 400K and latm

A

4.54 `g//lit`

B

3.54 `g//lit`

C

5.54 `g//lit`

D

None of these

Text Solution

Verified by Experts

The correct Answer is:
A
`underset(1-0.4)underset(1)(PCl_(5)) harr underset(0.4)underset(0)(PCl_(3(g))) + underset(0.4)underset(0)(Cl_(2(g)))`
Total moles at equilibrium = 1.4
`("Normal molar mass of" PCl_(5)=i+alpha)/("Exp. Molar mass of" PCl_(5)=1.4)`
`(208.5)/("Exp. molar mass")=1.4`
`implies` Exp. molar mass (or) Molar mass of mix = `(208.5)/(1.4)`
Now using `Pv=(wRT)/(M) implies P=(dRT)/(M)`
`d=(pM)/(RT)=(1 xx 208.5)/(1.4 xx 0.0821 xx 400)=4.54 g//lit`
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