The value of K p for the reaction, 2 SO 2( g )+ O 2( g ) leftharpoons 2 SO 3( g ) is 5 What will be the partial pressure of O 2 at equilibrium when equal moles of SO 2 and SO 3 are present at equilibrium?

Question

The value of K p for the reaction, 2 SO 2( g )+ O 2( g ) leftharpoons 2 SO 3( g ) is 5 What will be the partial pressure of O 2 at equilibrium when equal moles of SO 2 and SO 3 are present at equilibrium? (A) 0.5 (B) 0.3 (C) 0.2 (D) 0.1

Tardigrade Admin · Accepted Answer

2 SO 2+ O 2 leftharpoons 2 SO 3 K p =( p SO 32/ p SO 32 × p O 2)=5 ∵ n SO 2= n SO 3 ⇒ chi SO 2= chi SO 3 ⇒ P SO 2= p SO 3 ⇒ (1/ p O 2)=5 ⇒ P O 2=0.2

Q. The value of $K_{p}$ for the reaction,
$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ is $5$
What will be the partial pressure of $O_{2}$ at equilibrium when equal moles of $S O_{2}$ and $S O_{3}$ are present at equilibrium?

$0.5$

$0.3$

$0.2$

$0.1$

$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$
$K_{p} = \frac{p _{S O_{3}}^{2}}{p _{S O_{3}}^{2} \times p _{O_{2}}} = 5$
$∵ n_{S O_{2}} = n_{S O_{3}}$
$\Rightarrow χ S O_{2} = χ S O_{3} \Rightarrow P_{S O_{2}} = p_{S O_{3}}$
$\Rightarrow \frac{1}{p _{O_{2}}} = 5 \Rightarrow P_{O_{2}} = 0.2$

Q. The value of Kp​ for the reaction, 2SO2​(g)+O2​(g)⇌2SO3​(g) is 5 What will be the partial pressure of O2​ at equilibrium when equal moles of SO2​ and SO3​ are present at equilibrium?

0.5

0.3

0.2

0.1