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Equilibrium Constant Kc & Reaction Quotient Calculator

Compute the equilibrium constant Kc or reaction quotient Q from concentrations and coefficients, and see which way the reaction shifts.

Enter concentration and coefficient for each species; leave a row's concentration blank to skip it.

About this tool

The Equilibrium Constant & Reaction Quotient Calculator is a free, in-browser chemistry tool that evaluates the mass-action expression for a reversible reaction. Enter up to two reactants and two products, each with a molar concentration and a stoichiometric coefficient, and it returns Kc (using equilibrium concentrations) or Q (using current concentrations), along with the product and reactant terms that make up the ratio.

The expression is K (or Q) = Π[product]^coefficient ⁄ Π[reactant]^coefficient — every product concentration is raised to its coefficient and multiplied together for the numerator, every reactant likewise for the denominator, and the numerator is divided by the denominator. Leave a row's concentration blank to omit that species; a coefficient left blank defaults to 1. Concentrations are in mol/L and must be positive so the ratio stays finite.

Everything runs locally in your browser with no uploads. In Q mode you can also enter a known Kc, and the tool compares them to predict the shift by Le Chatelier's principle: Q < Kc means the reaction proceeds forward toward products, Q > Kc means it runs in reverse toward reactants, and Q = Kc means the system is already at equilibrium.

Frequently asked questions

How is the equilibrium expression built?
It is K = Π[product]^coeff ⁄ Π[reactant]^coeff. Each concentration is raised to its stoichiometric coefficient, products are multiplied for the top of the ratio and reactants for the bottom, then divided. Pure solids and liquids are simply left out by skipping their row.
What is the difference between Kc and Q?
They use the identical formula; the difference is the concentrations you feed in. Kc uses equilibrium concentrations and is a constant at a given temperature, while Q uses whatever the current concentrations are and tells you how far from equilibrium the system is.
How does it predict the direction of shift?
In Q mode, enter a known Kc and it compares: Q < Kc shifts forward toward products, Q > Kc shifts reverse toward reactants, and Q = Kc is at equilibrium. This is the quantitative form of Le Chatelier reasoning.
Why must concentrations be positive?
A zero or negative concentration would make the ratio zero, undefined, or infinite. Enter positive mol/L values for every species you include, and leave a concentration blank to exclude that species from the expression entirely.

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