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.

Question

Preston Franklin

Chemistry

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)

Know the Answer?

Javon Perkins · Answer 1

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