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

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

Step-by-step 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)=([SO_3]^2)/([SO_2]^2[O_2])`

`k_(eq)=([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.

Answer 2

15.41.

Step-by-step 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.