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Question

A compound exists in the gaseous phase both as a monomer (A) and as a dimer (A2). The molecular mass of A is 48 g mol1. In an experiment, 96 g of compound was confined in a vessel of volume 33.6 L and heated to 273C. Calculate the pressure (in atm, rounded off to the nearest integer) developed if the compound exists as a dimer to the extent of 50% by weight under these conditions.

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Solution

Since, the compound contains equal weight of A and A2,
Moles of A=962×148=1
and, Moles of A2=962×196=12
Total moles of A and A2 in the compound=1+12=32
From ideal gas equation,
PV=nRT
P×33.6=32×0.0821×546
P=2 atm

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