The equilibrium constant for the reaction,

$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$
at 1000 K is 3.5. What would be the partial pressure of oxygen gas if the equilibrium is found to have equal moles of $S O_{2}$ and $S O_{3}$ ?

Question

The equilibrium constant for the reaction,

$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$

at 1000 K is 3.5. What would be the partial pressure of oxygen gas if the equilibrium is found to have equal moles of $S O_{2}$ and $S O_{3}$ ?

TestHub · Accepted Answer

K p ​ = P S O 2 ​ 2 ​ × P O 2 ​ ​ ​ P S O 3 ​ 2 ​ ​ = 3.5 P S O 2 ​ ​ = P S O 3 ​ ​ i . e . P O 2 ​ ​ 1 ​ = 3.5 i . e . P O 2 ​ ​ = 0.285 a t m

Chemistry - Chemical Equilibrium Question with Solution | TestHub