View the step-by-step solution to:

# 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)

Since 
H 2 ( g ) + F2 ( g )    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 =...

### Why Join Course Hero?

Course Hero has all the homework and study help you need to succeed! We’ve got course-specific notes, study guides, and practice tests along with expert tutors.

### -

Educational Resources
• ### -

Study Documents

Find the best study resources around, tagged to your specific courses. Share your own to gain free Course Hero access.

Browse Documents