Answer :
Answer:
17.9 atm.
Explanation:
Okay, in the question above we are given the following information; the equilibrium constant (Kp) for the reaction= 2.40 × 10^3, and the initial partial pressure of NO= 36.1 atm.
The equilibrium constant,kp can be represented mathematically by using the formula below;
kp = P(N2) P(O2) / P^2 (NO).
The equation for the balanced Reaction is given below as;
2 NO <======> N2 + O2.
Therefore, at EQUILIBRIUM the partial pressure of NO = 36.1 - 2x and the partial pressure of N2 and O2 = x respectively.
So, let us go back to the formula for Calculating kp which is;
2.40 × 10^3 = x^2 / 36.1 - 2x.
Therefore, solving for the value of x in the question we have x = 17.9.
The partial pressure of the oxygen in the reaction mixture is 17.9 atm. Thus option C is correct.
From the balanced chemical equation, the partial pressure of NO is twice the partial pressure of Nitrogen and Oxygen.
Given, equilibrium constant = [tex]\rm 2.40\;\times\;10^3[/tex]
The partial pressure of system = 36.1 atm
Partial pressure of Nitrogen = x
Partial pressure of oxygen = x
Partial pressure of NO = 36.1 - 2x
Equilibrium constant = [tex]\rm \dfrac{[pN_2]\;[pO_2]}{[pNO]}[/tex]
[tex]\rm 2.40\;\times\;10^3[/tex] = [tex]\rm \dfrac{[x]\;[x]}{[36.1-2x]}[/tex]
[tex]\rm 2.40\;\times\;10^3[/tex] [tex]\times[/tex] (36.1 - 2x) = [tex]\rm x^2[/tex]
x = 17.9 atm.
Thus, the partial pressure of the oxygen in the reaction mixture is 17.9 atm. Thus option C is correct.
For more information about the partial pressure, refer to the link:
https://brainly.com/question/15075781