The gas-phase equilibrium of the oxidation of sulfur dioxide, shown here, has an equilibrium constant, K_p, value of 4.17 *10² at 200$\degree$C. If a closed vessel was filled with sulfur trioxide and the initial pressure of SO₃ was 0.033 atm at 200$\degree$C, what would be the final partial pressure of SO₃? 2SO₂(g) + O₂(g) 2SO₃(g)

Question

Quizplus · Accepted Answer

Since the equilibrium constant is greater than one, it means that the forward reaction is favored at equilibrium. Therefore, the concentration of sulfur trioxide will decrease and the concentration of sulfur dioxide and oxygen will increase until the equilibrium constant is reached. This implies that the final partial pressure of sulfur trioxide will be less than 0.033 atm.

The Gas-Phase Equilibrium of the Oxidation of Sulfur Dioxide, Shown °\degree°

The Gas-Phase Equilibrium of the Oxidation of Sulfur Dioxide, Shown $\degree$