Question

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.

Answer 1

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 2

Answer:

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

Explanation:

$2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)$

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

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

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

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

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

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

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