Respuesta :
Explanation:
Reaction equation for this reaction is as follows.
[tex]NO(g) + SO_{3}(g) \rightarrow NO_{2}(g) + SO_{2}(g)[/tex]
It is given that [tex]K_{p}[/tex] = 0.0118.
According to the ICE table,
[tex]NO(g) + SO_{3}(g) \rightarrow NO_{2}(g) + SO_{2}(g)[/tex]
Initial: 0.86 0.86 0 0
Change: -x -x +x +x
Equilibrium: 0.86 - x 0.86 - x x x
Hence, value of [tex]K_{p}[/tex] will be calculated as follows.
[tex]K_{p} = \frac{P_{NO_{2}} \times P_{SO_{3}}}{P_{NO} \times P_{SO_{3}}}[/tex]
0.0118 = [tex]\frac{x \times x}{(0.86 - x)^{2}}[/tex]
x = 0.084 atm
Thus, we can conclude that [tex]P_{NO_{2}}[/tex] is 0.084 atm.
0.084 atm is the equilibrium pressure of NO₂, if Kp for the reaction at this temperature is 0.0118.
How we calculate equilibrium constant from partial pressure (Kp)?
Equilibrium constant from partial pressure (Kp) can be calculated as:
Kp = [product of the concentration of products] / [product of the concentration of reactants]
Given chemical reaction can be expressed in terms of initial, change, equilibrium as follow:
NO(g) + SO₃(g) → NO₂(g) SO₂(g)
Initial: 0.86 0.86 0 0
Change: -x -x +x +x
Equilibrium: 0.86-x 0.86-x x x
From the above data expression for Kp is written as:
Kp = [NO₂] [SO₂] / [NO] [SO₃]
Kp = x.x / (0.86-x)²
In the question given value of Kp = 0.0118
Putting this value in the above equation, we get
0.0118 = x² / (0.86-x)²
On the solving the quadratic equation we get the value of x is 0.084 atm.
Hence, the equilibrium pressure of NO₂ is 0.084 atm.
To know more about Kp, visit the below link:
https://brainly.com/question/25651917
