A 0.100 mol sample of H2S is placed in a 10.0 L reaction vessel and heated to 1132°C. At equilibrium, 0.0285 mol H2 is present. Calculate the value of Kc for the reaction below at 1132°C.

2 H2S(g) 2 H2(g) + S2(g)

To calculate the value of Kc for the given reaction, we need to understand the concept of equilibrium and know the equilibrium expression.

The equilibrium constant, Kc, represents the ratio of the concentrations of products to the concentrations of reactants at equilibrium. For the given reaction:

2 H2S(g) ⇌ 2 H2(g) + S2(g)

The equilibrium constant expression can be written as:

Kc = [H2]^2 * [S2] / [H2S]^2

Given that the equilibrium concentrations are [H2S] = 0.100 mol and [H2] = 0.0285 mol, we need to determine the concentration of S2. Since we know that 2 moles of H2S produce 2 moles of H2 and 1 mole of S2, the concentration of S2 can be calculated by subtracting the concentration of H2 from the initial concentration of H2S.

[H2S] initial = 0.100 mol
[H2] = 0.0285 mol

Based on the stoichiometry of the reaction, 2 moles of H2S will produce 2 moles of H2. Therefore, the concentration of H2S at equilibrium will be:

[H2S] equilibrium = [H2S] initial - 2 * [H2]
= 0.100 mol - 2 * 0.0285 mol
= 0.100 mol - 0.0570 mol
= 0.0430 mol

Now, substituting the values into the equilibrium constant expression, we get:

Kc = ([H2]^2 * [S2]) / ([H2S]^2)
= (0.0285 mol)^2 * [S2] / (0.0430 mol)^2

Since the value of [S2] is not given, we cannot directly calculate the numerical value of Kc. However, based on the given information, you can calculate the value of Kc once you determine the concentration of S2.

Please note that the units of concentration should match for accurate calculations. If the concentration values are given in different units, you need to convert them to the same unit before plugging them into the equilibrium constant expression.