Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br₂ and NOBr

Question

Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br₂ and NOBr at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium..

2 NO(g) + Br₂(g) ⇌ 2 NOBr(g)

If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to solve for the partial pressure. Do not combine or simplify terms..

Kp= ---- =109

Based on your expression for Kp, solve for the equilibrium partial pressure of NO.

PNO= ___ atm

Answer 1

So Ina S.,

you use the same approach for this problem as for your other one, an ICE table. It looks like you are being given an equilibrium constant value expressed directly from partial pressures, doesn't it (as opposed to in units of M , for example). That should make it easy, sine you can just start writing table entries!

-- Cheers, -- Mr. d.