🤓 Based on our data, we think this question is relevant for Professor Xie's class at HOWARDCC.
We’re being asked to determine the equilibrium constant at 500˚C for this reaction:
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
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.
What is the value of the equilibrium constant at 500 °C for the formation of NH 3 according to the following equation?
N2(g) + 3H2(g) ⇌ 2NH3(g)
An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 °C was found to contain 1.35 M H 2, 1.15 M N2, and 4.12 × 10−1 M NH3.