The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N₂ and O₂ being injected into a 1.0-L container at 2500 k. The equilibrium constant at 2500 K is 3.6 × 10^–3. What was the composition of the reaction mixture after equilibrium was attained?

Data from exercise 12.33 

The following reaction establishes equilibrium at 2000 K:

If the reaction began with 0.100 mol L^–1 of N₂ and 0.100 mol L^–1 of O₂, what were the equilibrium concentrations of all species?

Transcribed Image Text:

N₂(g) + O₂(g) 2 NO K = 4.1 X 10-4