At some temperature, K = 337 for the gas phase reaction What is the concentratio

Question

At some temperature, K = 337 for the gas phase reaction

What is the concentration of HF in an equilibrium mixture established by adding 2.35 mol each of H2 and F2 to a 1.00 L container at this temperature?

[HF] = 4.31 (correct)

What would be the equilibrium concentration of HF if 2.54 mol HF were removed from the above equilibrium mixture?

So for this, I made a reaction table. Top row is initial values, middle is change, bottom row is final. This gave me final concentrations. I then set up a K equation.
I got the initial H_2 and F_2 values by using the equation for K, with [HF]=4.31.

K=[HF]^2/[H_2][F_2]
K=(1.27+2x)^2 / (.113-x)^2

solved for x, and got .0416, which then led me to [HF]=1.27+.0416=1.31, which was wrong.

Can someone please explain where I went wrong with this?

H_2 F_2 2HF .113 .113 1.27 -x -x +2x .113-x .113-x 1.27+2x At some temperature, K = 337 for the gas phase reaction H2 + F2 At some temperature, K = 337 for the gas phase rea 2HF What is the concentration of HF in an equilibrium mixture established by adding 2.35 mol each of H2 and F2 to a 1.00 L container at this temperature? [HF] = 4.31 (correct) What would be the equilibrium concentration of HF if 2.54 mol HF were removed from the above equilibrium mixture? So for this, I made a reaction table. Top row is initial values, middle is change, bottom row is final. This gave me final concentrations. I then set up a K equation. I got the initial H_2 and F_2 values by using the equation for K, with [HF]=4.31. K=[HF]^2/[H_2][F_2] K=(1.27+2x)^2 (.113-x)^2 solved for x, and got .0416, which then led me to [HF]=1.27+.0416=1.31, which was wrong. Can someone please explain where I went wrong with this?

Explanation / Answer

intailly [HF] value is wrong not 4.31 it's 43.14..

while next calucalating x value it's 0.039 not 0.0416 for [HF}= 4.31

337= [HF]^2/[2.35}*[2.35]

[HF] =43.14

337 = (1.27+2x)^2/(0.113-x)^2

x= 0.039

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