The following reaction has Kp = 109 at 25°C. 2 NO(g) + Br2(g) equilibrium reaction arrow 2 NOBr(g) If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.

The equilibrium partial pressure of NO is 0.0034 atm

Explanation:

For the given chemical equation:

The expression of for above equation follows:

We are given:

Equilibrium partial pressure of = 0.0159 atm

Equilibrium partial pressure of NOBr = 0.0768 atm

Putting values in above equation, we get:

Hence, the equilibrium partial pressure of NO is 0.0034 atm