Question

Consider the following reaction:

2SO₃(g) 2SO₂(g) + O₂(g).

If 0.100 moles of SO₃, 0.235 moles of SO₂, and 0.246 moles of O₂ are at equilibrium in a 13.0 L container at 1.23×103 K, the value of the equilibrium constant, Kp is ___.

A) 0.0355
B) 0.0672
C) 0.256
D) 0.112

Answer 1

The value of the equilibrium constant, Kp, for the given reaction is 0.0672.

Step-by-step explanation:

The equilibrium constant, Kp, for the reaction 2SO₃(g) → 2SO₂(g) + O₂(g) can be calculated using the given concentrations at equilibrium.

The equilibrium concentrations are [SO₃] = 0.100 M, [SO₂] = 0.235 M, and [O₂] = 0.246 M. Plugging these values into the equilibrium constant expression:

([SO₂]²[O₂]) / ([SO₃]²)

(0.235² * 0.246) / (0.100²)

Kp = 0.0672