Final answer:
To calculate the equilibrium constant, one must substitute the given equilibrium concentrations into the equilibrium constant expression and solve for the unknown. However, typos in the provided information imply the need for clarification before an accurate calculation can be made.
Step-by-step explanation:
The task at hand is to calculate the equilibrium constant (Kc) for a reaction given the equilibrium concentrations of the reactants and products. Given that the equilibrium constant expression relates the concentrations of the substances produced in the reaction to the substances that react according to a specific ratio dictated by the balanced equilibrium equation, we can use this information to calculate Kc.
Assuming that the reaction in question is N2 + 3H2 = 2NH3 and given equilibrium concentrations of [N2], [NH3], and [H2], with the values supplied as IN (Initial Nitrogen) being 1-0.071 M for [N2], I1 (Initial NH3) being 9.2×10^-9 M for [NH3], and the Kc given as 13.7, we can substitute these into the equilibrium expression Kc = [NH3]² / ([N2][H2]³), simplifying and solving for the unknown concentration of [H2].
However, it appears that the question provided has some typos and the numbers do not seem to fit the typical format for equilibrium concentrations or constant expressions. It is therefore recommended that the student clarify the information provided to ensure an accurate calculation can be performed.