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Question

A compound exists in the gaseous phase both as a monomer (A) and dimer $$(A_2)$$. The molar mass of A is 48. In an experiment, 96 g of the compound was confined in a vessel of volume 33.6 litre and heated to $$273^oC$$. Calculate the pressure (in atm) developed, if the compound exists as a dimer to the extent of 50% by mass under these conditions.


Solution

Since, A and $$A_2$$ are two states in the gaseous phase having their mass ratio 50%, i.e., 1:1

Mole of A$$=\cfrac {96}{2}\times \cfrac {1}{48}=1 \left (n=\cfrac {w}{M}\right )$$

Mole of $$A_2=\cfrac {96}{2}\times \cfrac {1}{96}=\cfrac {1}{2}$$

Total mole of A and $$A_2$$ are $$=1+\cfrac {1}{2}=\cfrac {3}{2}$$

Now, $$PV=nRT$$

$$ P\times 33.6=\cfrac {3}{2}\times 0.0821\times 546$$

$$ P=2 atm$$

Chemistry

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