For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.05-L rigid container are [H2] = 0.0523 M, [F2] = 0.0121 M, and [HF] = 0.450 M.
H2(g) + F2(g) 2 HF(g)
If 0.203 mol of F2 is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.
Concentration equilibrium constant, Kc = [HF]eq2 / [H2]eq[F2]eq
Kc = (0.450 M)2 / [(0.0523 M) * (0.0121 M)2]
Kc = 320
moles F2 added = 0.203 mol
concentration F2 added = (moles F2 added) / (volume of container)
concentration F2 added = (0.203 mol) / (5.05 L)
concentration F2 added = 0.0402 M
new concentration F2 = (0.0121 M) + (0.0402 M)
new concentration F2 = 0.0523 M
ICE table | H2 (g) | F2 (g) | 2 HF (g) | |
Initial conc. | 0.0523 M | 0.0523 M | 0.450 M | |
Change | -x | -x | +2x | |
Equilibrium conc. | 0.0523 M - x | 0.0523 M - x | 0.450 M + 2x |
Kc = [HF]eq2 / [H2]eq[F2]eq
320 = (0.450 M + 2x)2 / [(0.0523 M - x) * (0.0523 M - x)]
Solving for x, x = 0.0244 M
equilibrium concentration H2 = 0.0523 M - x
equilibrium concentration H2 = 0.0523 M - 0.0244 M
equilibrium concentration H2 = 00279 M
equilibrium concentration F2 = 0.0523 M - x
equilibrium concentration F2 = 0.0523 M - 0.0244 M
equilibrium concentration F2 = 00279 M
equilibrium concentration HF = 0.450 M + 2x
equilibrium concentration HF = 0.450 M + 2 * (0.0244 M)
equilibrium concentration HF = 0.499 M
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