How does the Equilibrium Constant Kc work?

Write the balanced equation Then: Kc = [Products]^coefficients / [Reactants]^coefficients Then: Solids and pure liquids are excluded (activity = 1) Then: Reaction quotient Q compared to Kc tells direction of reaction.

Can you give an example of how to use the Equilibrium Constant Kc?

Example: Input N₂ + 3H₂ ⇌ 2NH₃ at equilibrium: [N₂]=0.1, [H₂]=0.2, [NH₃]=0.5M gives a result of Kc = [0.5]²/([0.1][0.2]³) = 312.5 (Large Kc → strong product favour).

Is the Equilibrium Constant Kc free to use?

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How accurate is the Equilibrium Constant Kc?

Our Equilibrium Constant Kc uses verified mathematical formulas and is accurate to multiple decimal places. Results are calculated in real-time using the same methods used by professionals.

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Equilibrium Constant Kc

⚗️Equilibrium Constant (Kc)

Product concentrations (comma separated, mol/L)

Reactant concentrations (comma separated, mol/L)

The equilibrium constant (Kc) quantifies the ratio of product to reactant concentrations at equilibrium for a reversible reaction. Kc > 1 means products are favoured; Kc < 1 means reactants are favoured.

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Did You Know?

The Haber process (N₂ + 3H₂ → 2NH₃) uses Le Chatelier's principle: high pressure and moderate temperature (despite less favourable equilibrium) maximize ammonia output and productivity.

References

›Equilibrium constant — Wikipedia

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Equilibrium Constant Kc

⚗️Equilibrium Constant (Kc)

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⚗️Equilibrium Constant (Kc)