Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 723.0 K: [N2(g)] = 2.936 mol/L, [H2(g)] = 2.933 mol/L, [NH3(g)] = 3.443 mol/L.
N2(g)+3H2(g) = 2NH3(g)
Look at the ClF problem above and see if you can do this one.
To calculate the value of the equilibrium constant (Kc) for the given reaction, you need to use the equilibrium concentrations of the reactants and products. In this case, the equilibrium concentrations are as follows:
[N2(g)] = 2.936 mol/L
[H2(g)] = 2.933 mol/L
[NH3(g)] = 3.443 mol/L
First, write the expression for the equilibrium constant (Kc) based on the balanced equation:
Kc = [NH3(g)]^2 / ([N2(g)] * [H2(g)]^3)
Now, substitute the given equilibrium concentrations into the equation:
Kc = (3.443)^2 / (2.936 * 2.933^3)
Simplify the equation:
Kc = 11.853 / (2.936 * 48.309)
Now, calculate the value of Kc:
Kc ≈ 0.084
Therefore, the value of the equilibrium constant (Kc) for the given reaction at 723.0 K is approximately 0.084.