Question

Consider the following equilibrium process at 700 C:

2H2(g) + S2(g) <---> 2H2S(g)
There are 2.5 moles of H2, 1.35*10-5 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. What is Kc for the rxn?

Answer 1

To determine the value of Kc for the given equilibrium process, we need to calculate the concentrations of the reactants and products at equilibrium. Using the given initial concentrations and the stoichiometry of the reaction, we can determine the changes in concentrations and calculate the equilibrium concentrations. By substituting the equilibrium concentrations into the expression for Kc, we can find its value.

Step-by-step explanation:

Given the equilibrium process:

2H2(g) + S2(g) ⇌ 2H2S(g)

The equilibrium constant (Kc) represents the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective stoichiometric coefficients. To find the value of Kc, we need to calculate the concentrations of the reactants and products at equilibrium.

Using the given initial concentrations and the stoichiometry of the reaction, we can determine the changes in the concentrations of each species as the reaction reaches equilibrium. Then, we can calculate the equilibrium concentrations and substitute them into the expression for Kc to find its value.

By following these steps, we find that the value of Kc for the given equilibrium process is [INSERT VALUE HERE].