For the reaction: 2NO(g) + H2(g) <=> N2O(g) + H2O(g) + energy
Write the equilibrium constant expression for the reaction.
This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of H2 is 3.00 mol/L, the concentration of N2O is 4.00 mol/L, and the concentration of H2O is 1.25 mol/L. Using the balanced chemical equation, calculate the equilibrium constant for this system.
See your post above.
The equilibrium constant expression for the reaction can be written using the concentrations of the reactants and products. In the given reaction, the equilibrium constant expression is as follows:
Kc = [N2O(g)][H2O(g)] / [NO(g)]^2[H2(g)]
To calculate the equilibrium constant (Kc) for this system, we substitute the given concentrations into the equation:
Kc = (4.00 mol/L) * (1.25 mol/L) / (1.75 mol/L)^2 * (3.00 mol/L)
Kc = 5.0 / 3.9375
Kc = 1.27
Therefore, the equilibrium constant for this system is 1.27.