Question

The oxidation of sulfur dioxide by oxygen to sulfur trioxide has been implicated as an important step in the formation of acid rain: 2 SO2(g) + O2(g) ⇌ 2 SO3(g). If the equilibrium partial pressures of SO2, O2, and SO3 are 0.564 atm, 0.102 atm, and 0.333 atm respectively at 1000 K, what is K p at that temperature?

Answer 1

Answer:

The value of the equilibrium constant $K_p$ at this temperature is 3.42.

Explanation:

Partial pressure of the sulfur dioxide =$p_1=0.564 atm$

Partial pressure of the oxygen gas =$p_2=0.102 atm$

Partial pressure of the sulfur trioxide =$p_3=0.333$

$2 SO_2(g) + O_2(g)\rightleftharpoons 2 SO_3(g)$

The expression of an equilibrium constant is given by :

$K_p=\frac{(p_3)^2}{(p_1)^2\times p_2}$

$K_p=\frac{(0.333 atm)^2}{(0.564 atm)\times (0.102 atm)}=3.42$

The value of the equilibrium constant $K_p$ at this temperature is 3.42.