Chemistry Forum

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.

Kp = Kc * RT ^(Δn)

Δn = moles gaseous products - moles gaseous reactants

In your case you have only gaseous products.

Kp = pNH₃* pH₂S

https://byjus.com/question-answer/kp-an ... ure-12-5k/

Thanks a lot, as there are two gaseous products, so Δn will be 2, right??

Correct. 2-0 = 2