🤓 Based on our data, we think this question is relevant for Professor Czernuszewicz's class at UH.
We’re being asked to determine Kp at 500 K for this reaction:
2NO (g) + Cl2 (g) ⇌ 2NOCl (g)
Recall that the equilibrium constant is the ratio of the products and reactants.
We use Kp when dealing with pressure.
*Note that solid and liquid compounds are ignored in the equilibrium expression.
2NO (g) + Cl2 (g) 2NOCl (g)
is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.50×10−2 atm , 0.175 atm , and 0.27 atm for NO, Cl2, and NOCl, respectively.
Calculate Kp for this reaction at 500.0 K.