At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g)
is Kc=15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.
Left No net reaction Right

Answers are in the explanation.

Explanation:

Given concentrations are:

SO₂ = 0.20M O₂ = 0.60M SO₃ = 0.60MSO₂ = 0.14M O₂ = 0.10M SO₃ = 0.40M And SO₂ = 0.90M O₂ = 0.50M SO₃ = 0.10M

In the reaction:

2SO₂(g) + O₂(g) ⇄ 2SO₃(g)

Kc is defined as:

Kc = 15 = [SO₃]² / [O₂] [SO₂]²

Where concentrations of each species are equilbrium concentrations.

Also, you can define Q (Reaction quotient) as:

Q = [SO₃]² / [O₂] [SO₂]²

Where concentrations of each species are ACTUAL concentrations.

If Q > Kc, the reaction will shift to the left until Q = Kc;

If Q < Kc, the reaction will shift to the right until Q = Kc

If Q = Kc, there is no net reaction because reaction would be en equilibrium.

Replacing with given concentrations:

Q = [0.60M]² / [0.60M] [0.20M]² = 15; Q = Kc → No net reactionQ = [0.40M]² / [0.10M] [0.14M]² = 82; Q > Kc, → Reaction will shift to the leftQ = [0.10M]² / [0.50M] [0.90M]² = 0.015; Q < Kc → Reaction will shift to the right

The answer is yes b ffgnbsfgnbnfgbnfgsnb

Ithink 2 is the correct