Ask Question
22 February, 07:32

At 1000 K, a sample of pure NO2 gas decomposes. 2 NO2 (g) equilibrium reaction arrow 2 NO (g) + O2 (g) The equilibrium constant KP is 158. Analysis shows that the partial pressure of O2 is 0.99 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture.

+2
Answers (1)
  1. 22 February, 07:33
    0
    0.1575 atm

    Explanation:

    we have that equilibrium constant Kp = (PNO) ₂PO₂ / (PNO₂) ₂

    and it is given to be 158

    ==> Kp = (PNO) ₂PO₂ / (PNO₂) ₂ = 158

    we also have that the partial pressure of O2 (PO₂) = 0.99 atm

    Therefore,

    PO₂ = 0.99 atm = => PNO = 2 (0.99 atm) = 1.98 atm (based on the stoichiometry)

    ==> PNO₂ = √ ((PNO) ₂PO₂ / 158) atm = √ ((1.98) * 2 (0.99) / 158) atm = 0.1575 atm
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “At 1000 K, a sample of pure NO2 gas decomposes. 2 NO2 (g) equilibrium reaction arrow 2 NO (g) + O2 (g) The equilibrium constant KP is 158. ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers