🤓 Based on our data, we think this question is relevant for Professor Davis' class at OLE MISS.
Consider the reaction:
2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K
In a reaction mixture at equilibrium, the partial pressure of NO is 126 torr and that of Br2 is 159torr .
What is the partial pressure of NOBr in this mixture?
We’re being asked to determine the equilibrium partial pressure of NOBr for the reaction:
2NO(g) + Br2(g) ⇌ 2NOBr(g) Kp = 28.4 at 298 K
Recall that the equilibrium constant is the ratio of the products and reactants.
We use Kp when dealing with pressure and Kc when dealing with concentration:
Note that solid and liquid compounds are ignored in the equilibrium expression.