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The reaction for the formation of gaseous hydrogen fluoride has an equilibrium constant of KC = 1.1510^2 at a given temperature. Assuming that the...

The reaction for the formation of gaseous hydrogen fluoride has an equilibrium constant of KC = 1.15×10^2 at a given temperature. Assuming that the reaction starts by adding 3.00 moles of each component (H2, F2, and HF) to a 1.5-L reactor, calculate the equilibrium concentration of hydrogen fluoride.

H2(g) + F2(g) <--> 2 HF(g)

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Hi, Please find the... View the full answer

5.doc

Since ˆˆ
H 2 ( g ) + F2 ( g ) ˆ ˆ ˆˆ 2 HF ( g )
I( M)
C
Eq 3.0
=2
1.5
-x 2 2 -x +2x ( 2-x ) ( 2-x ) K c =1.15×10 2 2x ( 2+2x )
=
2
( 2-x ) 2 By solving - x =1.528 M
Therefore - [ HF] = 2x =...

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