At some temperature, K = 292 for the gas phase reaction What is the concentratio

Question

At some temperature, K = 292 for the gas phase reaction

What is the concentration of HF in an equilibrium mixture established by adding 4.20 mol each of H2 and F2 to a 1.00 L container at this temperature?

What would be the equilibrium concentration of HF if 6.02 mol HF were removed from the above equilibrium mixture?

At some temperature, K = 292 for the gas phase reaction What is the concentration of HF in an equilibrium mixture established by adding 4.20 mol each of H2 and F2 to a 1.00 L container at this temperature? What would be the equilibrium concentration of HF if 6.02 mol HF were removed from the above equilibrium mixture?

Explanation / Answer

(a) H2 + F2 ---> 2 HF

at equilibrium

[H2] = 4.2 - x

[F2] = 4.2 - x

[HF] = 2x

K = [HF]^2 / ([H2]*[F2]) = (2x)^2 / (4.2-x)^2 = 292

so 2x / (4.2-x) = 17.08

solve then

x = 3.75 M and [H2] = [F2] = 0.45 M ; [HF] = 2*3.75 = 7.5 M

(b) at new equilibrium

[H2] = [F2] = 0.45-x and [HF] = 7.5 - 6.02 + 2x = 1.48 + 2x

(1.48+2x) / (0.45-x) = 17.08

solve

x = 0.32 M and [H2] = [F2] = 0.45-0.32 = 0.13 M ; [HF] = 1.48 + 2(0.32) = 2.12 M

All the best

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