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An equilibrium mixture of so2, o2, and so3 gases at 1500k is determined to consist of 0.344 mol/l so2, 0.172 mol/l o2, and 0.56 mol/l so3. what is the equilibrium constant for the system at this temperature? the balanced equation for this reaction is 2so2(g o2(g « so3(g.

Respuesta :

superman1987

Answer:

15.41.

Explanation:

  • From the balanced equation:

2SO₂(g) + O₂(g) ⇄ 2SO₃(g).

The equilibrium constant = Keq = [SO₃]²/[SO₂]²[O₂].

∴ Keq = [SO₃]²/[SO₂]²[O₂] = (0.56 mol/L)²/(0.344 mol/L)²(0.172 mol/L) = 15.41.

Answer:

The equilibrium constant for the system at this temperature is 15.4074.

Explanation:

[tex]2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)[/tex]

Concentration of [tex][SO_2][/tex] = 0.344 mol/L

Concentration of [tex][O_2][/tex] = 0.172 mol/L

Concentration of [tex][SO_3][/tex] = 0.56 mol/L

The equilibrium constant of the given equilibrium equation will be given as:

[tex]k_{eq}=\frac{[SO_3]^2}{[SO_2]^2[O_2]}[/tex]

[tex]k_{eq}=\frac{[0.56 mol/L]^2}{[0.344 mol/L]^2[0.172 mol/L]}=15.4074[/tex]

The equilibrium constant for the system at this temperature is 15.4074.

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