On analysis, an equilibrium mixture for the reaction 2H2S(g) LaTeX: \longleftrightarrow⟷ 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. Group of answer choices

The equilibrium constant Kc = 3.2

Explanation:

Step 1: Data given

Number of moles H2S = 1.0 moles

Number of moles H2 = 4.0 moles

Number of moles S2 = 0.8 moles

Volume = 4.0 L

Step 2: The balanced equation

2H2S(g) ⟷ 2H2(g) + S2(g)

Step 3: Calculate concentration

Concentration = moles / volume

[H2S] = 1.0 moles / 4.0 L

[H2S] = 0.25 M

[H2] = 4.0 moles / 4.0 L

[H2]= 1.0 M

[S2] = 0.80 moles / 4.0 L

[S2] = 0.20 M

Step 4: Calculate Kc

Kc = [S2][H2]² / [H2S]²

Kc = (0.20 * 1.0²) / 0.25²

Kc = 3.2

The equilibrium constant Kc = 3.2

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .