The Power of Equilibrium Constants in Chemical Reactions

How can we calculate the equilibrium constant for a chemical reaction?

For the equilibrium CH4(g) + 2H2S(g) "CS2(g) + 4H2(g), what are the concentrations at equilibrium?

Calculating Equilibrium Constant

The equilibrium constant (Kc) for the given reaction is approximately 0.04374.

By using the concentrations of the reactants and products at equilibrium, we can calculate Kc with the formula

Equilibrium constants play a crucial role in understanding chemical reactions. They provide valuable insights into the distribution of products and reactants at equilibrium.

In the example of the reaction CH4(g) + 2H2S(g) "CS2(g) + 4H2(g), we are given the concentrations at equilibrium as [CH4] = 0.3322M, [H2S] = 0.6644M, [CS2] = 0.0678M, and [H2] = 0.2712M at 1400.0 K.

To calculate the equilibrium constant (Kc) for this reaction, we use the formula:

Kc = ([CS2][H2]^4) / ([CH4][H2S]^2)

Substituting the given concentrations into the formula, we find:

Kc = (0.0678 M)(0.2712 M)^4 / (0.3322 M)(0.6644 M)^2 = 0.04374

Therefore, the equilibrium constant (Kc) for the given reaction is approximately 0.04374.

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