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 are 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 = (NOBr)^2 / ((NO)^2 * (Br2))
109 = (0.0768)^2 / ((x)^2 * (0.0159))