On analysis, an equilibrium mixture for the reaction 2H2S (g) 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.

Question

Chemistry

Alicia Stanton

4 November, 11:15

On analysis, an equilibrium mixture for the reaction 2H2S (g) 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.

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Answers (1)

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Bennett Lin · Answer 1

The equilibrium constant for this reaction is 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 = 0.80 moles

Volume = 4.0 L

Step 2: The balanced equation

2H2S (g) ⇆ 2H2 (g) S2 (g)

Step 3: Calculate molarity

[H2] = 4.0 moles / 4.0 L = 1.0 M

[S2] = 0.80 moles / 4.0 L = 0.20 M

[H2S] = 1.0 moles / 4.0 L = 0.25 M

Step 4: Calculate Kc

Kc = [H2]²[S2] / [H2S]²

Kc = (1.0²*0.20) / 0.25²

Kc = 0.2 / 0.0625

kC = 3.2

The equilibrium constant for this reaction is 3.2