contestada

The elementary reaction 2H20(g)<--->2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2, and O2 reach 0.0900 atm, 0.00450 atm, and 0.00100 atm, respectively. What is the value of the equilibrium constant at this temperature?

Respuesta :

Answer : The value of equilibrium constant (Kp) is, [tex]2.5\times 10^{-6}[/tex]

Explanation :  Given,

Partial pressure of [tex]H_2O[/tex] = 0.0900 atm

Partial pressure of [tex]H_2[/tex] = 0.00450 atm

Partial pressure of [tex]O_2[/tex] = 0.00100 atm

The given chemical reaction is:

[tex]2H_2O(g)\rightarrow 2H_2(g)+O_2(g)[/tex]

The expression for equilibrium constant is:

[tex]K_p=\frac{(p_{H_2})^2\times (p_{O_2})}{(p_{H_2O})^2}[/tex]

Now put all the given values in this expression, we get:

[tex]K_p=\frac{(0.00450)^2\times (0.00100)}{(0.0900)^2}[/tex]

[tex]K_p=2.5\times 10^{-6}[/tex]

Thus, the value of equilibrium constant (Kp) is, [tex]2.5\times 10^{-6}[/tex]