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.
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Taylor's class at CLEMSON.