Respuesta :
Answer: The initial partial pressures of [tex]NO[/tex] and [tex]Cl_2[/tex] is 139.4 torr.
Explanation:
The equilibrium reaction is
[tex]2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)[/tex]
initially conc. p p 0
At eqm. p-2x p-x 2x
Given: [tex]p_{NOCl}= 2x= 115torr[/tex]
[tex]x=57.5 torr[/tex]
The expression for equilibrium constant is :
[tex]K_p=\frac{p_{NOCl}^2}{p_{NO}^2\times p_{Cl_2}}[/tex]
[tex]p_{NOCl}[/tex] = 2x =115 torr
[tex]p_{NO}[/tex] = (p-2x) = p-115 torr
[tex]p_{Cl_2}[/tex] = (p-x)= p-57.5 torr
Now put all the given values in this expression, we get
[tex]0.27=\frac{(115)^2}{(p-115)^2\times (p-57.5)}[/tex]
[tex]p=139.4torr[/tex]
Therefore, the initial partial pressures of [tex]NO[/tex] and [tex]Cl_2[/tex] is 139.4 torr.
NO and Cl₂ initially at 139 torr react to form NOCl at 115 torr at equilibrium.
What is the chemical equilibrium?
Chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time.
- Step 1: Write the balanced equation.
2 NO(g) + Cl₂(g) ⇄ 2 NOCl(g) Kp = 0.27 at 700 K
- Step 2: Make an ICE chart.
We will use letters for unknown pressures.
2 NO(g) + Cl₂(g) ⇄ 2 NOCl(g)
I x x 0
C -2y -y +2y
E x-2y x-y 2y
Since the pressure of NOCl at equilibrium is 115 torr, we can conclude that:
2y = 115 torr
y = 57.5 torr
The pressures at equilibrium are:
pNO = x - 115
pCl₂ = x - 57.5
pNOCl = 115
We will put these values in the equilbrium constant Kp.
Kp = 0.27 = 115² / (x - 115)² × (x - 57.5)
x = 139 torr
NO and Cl₂ initially at 139 torr react to form NOCl at 115 torr at equilibrium.
Learn more about chemical equilibrium here: https://brainly.com/question/5081082
