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Solid NH4HS is introduced into an evacuated flask at 24 ∘C. The following reaction takes place: NH4HS(s)⇌NH3(g)+H2S(g) At equilibrium the total pressure (for NH3 and H2S taken together) is 0.614 atm.

Respuesta :

Answer:

0.09425

Explanation:

The reactant is in solid phase and therefore has zero partial pressure.

The products have the same mole ratio (1:1) and will have the same partial pressure = 1/2 × 0.614 atm = 0.307 atm

Kp =  (NH3)(H2S) = 0.09425

The value of Kp is 0.09425

Calculation of value of Kp:

Here

The reactant should be a solid phase and due to this it contains zero partial pressure.

And,

The products have the similar mole ratio (1:1) and will have the same partial pressure = 1/2 × 0.614 atm

= 0.307 atm

Now

Kp =  (NH3)(H2S)

= 0.09425

Learn more about the pressure here: https://brainly.com/question/13511474

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