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Question

The degree of dissociation is 0.4 at 400K and 1 atm for the gaseous reaction.
PCl5PCl3+Cl2. Assuming ideal behaviour of all the gases. Calculate the density of the equilibrium mixture at 400K and 1 atm Pressure.

A
4.53 g/L
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B
9.26 g/L
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C
1.25 g/L
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D
7.28 g/L
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Solution

The correct option is A 4.53 g/L

We have, PCl5PCl3+Cl2

Initial mole , 1 0 0

Mole at equilibrium 10.4 0.4 0.4

Total mole at equilibrium = 10.4+0.4+0.4=1.4

NormalMPCl5ObservedMPCl5=1+α=1.4

Therefore, Observed MPCl5=208.51.4

At equilibrium, PV=(wm)RT

Or, wV=PmRT

density= (1×208.5)(1.4×0.0821×400)

density= 4.53gL


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