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At a certain temperature, the K p for the decomposition of H 2 S is 0.743 . H 2 S ( g ) − ⇀ ↽ − H 2 ( g ) + S ( g ) Initially, only H 2 S is present at a pressure of 0.298 atm in a closed container. What is the total pressure in the container at equilibrium?

Respuesta :

Answer: The total pressure in the container at equilibrium is 0.526 atm

Explanation:

Equilibrium constant for a reaction is the ratio of concentration of products to the concentration of reactants each raised to the power its stoichiometric coefficients.

For the given reaction:

                 [tex]H_2S(g)\rightleftharpoons H_2(g)+S(g)[/tex]

initilal:    0.298 atm            0        0

at eqm    (0.298-x) atm     x atm    x atm

Total pressure  at eqm = (0.298-x) + x + x = 0.298 + x

Equilibrium constant is given as:

[tex]K_{p}=\frac{[H_2]\times [S]}{[H_2S]}[/tex]

[tex]0.743=\frac{(x)\times (x)}{(0.298-x)}[/tex]

[tex]x=0.228atm[/tex]

Thus (0.298 + x) = (0.298+0.228) atm = 0.526 atm

The total pressure in the container at equilibrium is 0.526 atm

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