Question:
At a certain temperature, 0.4211 mol of N, and 1.541 mol of H, are placed in a 5.00 L container. N₂(g) + 3H₂ ⥨ 2NH3(g) At equilibrium, 0.1401 mol of N, is present. Calculate the equilibrium constant
Last updated: 7/26/2022
![At a certain temperature, 0.4211 mol of N, and 1.541 mol of H, are placed in a 5.00 L container.
N₂(g) + 3H₂ ⥨ 2NH3(g)
At equilibrium, 0.1401 mol of N, is present. Calculate the equilibrium constant](https://media.kunduz.com/media/sug-question/raw/76626137-1658823003.1741235.jpeg?h=512)
At a certain temperature, 0.4211 mol of N, and 1.541 mol of H, are placed in a 5.00 L container. N₂(g) + 3H₂ ⥨ 2NH3(g) At equilibrium, 0.1401 mol of N, is present. Calculate the equilibrium constant, Kc.