Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Ashfakur Rahman on January 09, 2024, 01:18:10 AM
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Please solve the following problem:
Consider the following equilibrium at 395 K:
NH4HS(s) ⥫⥬ NH3 (g) + H2S(g)
The partial pressure of each gas is 0.265 atm. Calculate KP and Kc for the reaction.
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Please read the forum rules (https://www.chemicalforums.com/index.php?topic=65859.0), you have to show your efforts at answering the question to receive help.
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@ OP Bear in mind that at the given temperature NH4SH will be a gas.
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Probably you are right.
But it is written NH4HS(s)
s means solid.
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Yes, a rather contradictory question.
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Consider the following equilibrium at 395 K:
NH4HS(s) ⥫⥬ NH3 (g) + H2S(g)
The partial pressure of each gas is 0.265 atm. Calculate KP and Kc for the reaction.
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Calculate Kp first using Kp expression in which do not include solid NH4SCN.
Kp = KC (RT)Δn