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Question

The equilibrium constant of the reaction A2(g)+B2(g)2AB(g) at 100 is 50. If a one litre flash containing one mole of A2 is connected to a two litre flask containing two moles of B2 how many moles will be formed at 373K?

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Solution


A2(g)+B2(g)2AB(g)K=50
Above situation is initial picture and allowed to react
Total Volume =1+2=3 lit.
A2(g)+B2(g)2AB(g)K=50
At 1 2 0
t=0
At 1α 2(1α) 2α
t=teq
concentration =massvolinlit
At
Eq'b 1α3 2(1α)3 2α/3
conc. of of of
A2 B2 AB
K=(2α/3)22(1α)3×(1α)3=50
=2α2(1α)2=50=α1α=5
α=5/6
Hence 2α=5/3 moles of AB is formed.

1064119_789659_ans_cd96c9295b574b2aa67a10c86a87ffa7.jpg

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