Answer:
0.012
Explanation:
Let's consider the following reaction.
SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g)
We can find the concentrations at equilibrium using an ICE Chart.
SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g)
I 2.1 × 10⁻² 0 0
C -x +x +x
E 2.1 × 10⁻²-x x x
We know that the concentration of Cl₂ at equilibrium is 1.1 × 10⁻² M, so x = 1.1 × 10⁻² M.
The concentrations at equilibrium are:
[SO₂Cl₂] = 2.1 × 10⁻²-x = 2.1 × 10⁻²- 1.1 × 10⁻² = 1.0 × 10⁻² M
[SO₂] = [Cl₂] = x = 1.1 × 10⁻² M
The concentration equilibrium constant (Kc) is:
Kc = [SO₂] × [Cl₂] / [SO₂Cl₂]
Kc = 1.1 × 10⁻² × 1.1 × 10⁻² / 1.0 × 10⁻²
Kc = 0.012
