The equilibrium concentrations for the reaction between SO2 and O2 to form SO3 at a certain temperature are given in the table below. Determine the
equilibrium constant and whether the reaction favors reactants, products, or
neither at this temperature.
O(g) +250 (9)
2250 (9)
[02]
[SO2)
[S03)
1.2 M
0.80 M
1.9 M
A. K = 4.7; product favored
B. K = 0.51; product favored
C. K = 0.51; reactant favored
o
D. K= 4.7; reactant favored

A. K = 4.7; product favored

Explanation:

Step 1: Write the balanced reaction at equilibrium

O₂(g) + 2 SO₂(g) ⇄ 2 SO₃(g)

Step 2: Calculate the concentration equilibrium constant (Kc)

The equilibrium constant, Kc, is the ratio of the equilibrium concentrations of products over the equilibrium concentrations of reactants each raised to the power of their stoichiometric coefficients.

Kc = [SO₃]² / [SO₂]² × [O₂]

Kc = 1.9² / 0.80² × 1.2 = 4.7

When Kc > 1, the products are favored.

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~courtney

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