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.

the old alchemists made significant contributions to science even though there starting premises were off a bit. their conclusions after failure would steer them into better directions for investigation. science is no more than close observation and the initial mistakes result in rethinking and retrying experiments.