Given: 2SO₂(g) + O₂(g) $f$
2SO₃(g)
At equilibrium at a certain temperature,The concentrations of SO₃(g) ,SO₂(g) ,And O₂(g) Are 0.12 M,0.86 M,And 0.33M,Respectively.
Calculate the value of K_c for this reaction.

Question

Given: 2SO₂(g) + O₂(g)

f

2SO₃(g)
At equilibrium at a certain temperature,The concentrations of SO₃(g) ,SO₂(g) ,And O₂(g) Are 0.12 M,0.86 M,And 0.33M,Respectively.
Calculate the value of K_c for this reaction.

Quizplus · Accepted Answer

The equilibrium constant $K_c$ is calculated using the formula $K_c = \frac{[products]}{[reactants]}$ for the given reaction. Here, the reaction is $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$. Thus, $K_c = \frac{[SO_3]^2}{[SO_2]^2[O_2]}$. Substituting the given concentrations, $K_c = \frac{(0.12)^2}{(0.86)^2(0.33)} = 0.059$.

Given: 2SO2(g) + O2(g) fff 2SO3(g) at Equilibrium at a Certain Temperature,The Concentrations of a Certain

Given: 2SO₂(g) + O₂(g) $f$ 2SO₃(g)
at Equilibrium at a Certain Temperature,The Concentrations of a Certain