Question

The reaction 2 NO(g) + Br2(g) equilibrium reaction arrow 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0155 atm and the equilibrium partial pressure of NOBr is 0.0763 atm, calculate the partial pressure of NO at equilibrium.

Answer 1

See explanation below

Step-by-step explanation:

To know this, we need to write again the reaction, and then, write the expression for the equilibrium constant Kp:

2NO + Br₂ <------> 2NOBr Kp = 109

The Kp expression for this reaction is:

Kp = PpNOBr² / PpNO² * PpBr₂

Solving for the NO we have:

PpNO² = PpNOBr² / PpBr₂ * Kp

All we have to do now, is replace the given values:

PpNO² = (0.0763)² / (0.0155) * 109

PpNO² = 3.45x10⁻³

PpNO = √3.45x10⁻³

PpNO = 0.0587 atm