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.
This looks so straight forward. What is your problem with this. Exactly what do you not understand.
To write the equilibrium constant expression, we start with the balanced chemical equation:
2NO(g) + H2(g) <=> N2O(g) + H2O(g)
The equilibrium constant expression is written as:
Kc = [N2O(g)][H2O(g)] / [NO(g)]^2[H2(g)]
Now, to calculate the equilibrium constant for this system, we need to substitute the given concentrations into the equilibrium constant expression:
Kc = (4.00 mol/L)(1.25 mol/L) / (1.75 mol/L)^2(3.00 mol/L)
Kc = (5.00 mol^2/L^2) / (3.06 mol^2/L^2)
Kc = 1.63
Therefore, the equilibrium constant (Kc) for this system at 25°C is approximately 1.63.