Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO₂(g) . 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) K_c = 1.7 × 10⁸M^-1
[SO₃]_eq = 0.0034 mol L^-1 [O₂]_eq = 0.0018 mol L^-1

Question

Quizplus · Accepted Answer

Using the equilibrium constant and equilibrium concentrations, we can set up an ICE table to solve for the equilibrium concentration of SO₂(g): 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) I 0.0018 mol 0.0018 mol C - 2x -x +2x E 0.0018 - 2x 0.0018 - x 2x K = ([SO₃]_eq)2[O₂]_eq]/[SO₂]2 1.7 × 10⁸M^-1 = (2x)2/(0.0018 - 2x)2 Assuming x is small relative to 0.0018, we can simplify the equation: 1.7 × 10⁸M^-1 ≈ (2x)2/0.00182 x ≈ 6.1 × 10^-6 Therefore, the equilibrium concentration of SO₂(g) is approximately 6.1 × 10^-6 mol/L, or choice C.

Consider the Following Reaction, Equilibrium Concentrations, and Equilibrium Constant at a Particular