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## Homework Statement

What is the value of Kc for the reaction H2(g) + F2(g) <=> 2HF(g) given that when 0.010 mol H2 and 0.050 mol F2 are added to a 1.00 L container, 0.0125 mol HF is present at equilibrium.

## Homework Equations

## The Attempt at a Solution

I'm confused about how to set up the ICE chart in this scenario. We have

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

.01....... (.05) ....... 0

-x ......-x ........... 2x

.01-x.....(.05-x) ..... (.0125)

2x = .0125, x = .00625,

[.0125] ^2 / [.01 - .00625] [ .05-.00625] = 9.3 x 10 ^-6

Which is the incorrect answer, 9.51 ^-1 is right but I'm not sure how to get there. Any help would be appreciated.

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