Gaseous StateHard
Question
A compound exists in the gaseous phase both as monomer (A) and dimer (A2). The atomic mass of A is 48 and molecular mass of A2 is 96. In an experiment 96 g of the compound was confined in a vessel of volume 33.6 litre and heated to 273oC. The pressure developed if the compound exists as dimer to the extent of 50 % by weight under these conditions will be :
Options
A.1 atm
B.2 atm
C.1.5 atm
D.4 atm
Solution
Since A and A2 are two states in gaseous phase having their wt ratio 50% i.e. 1 : 1
moles of A =
= 1 Moles of A2 = 
Total mole = 3/2
P = nRT/V.
moles of A =
= 1 Moles of A2 = Total mole = 3/2
P = nRT/V.
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