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Equilibrium Constant Formula:
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The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at chemical equilibrium. It indicates the extent to which a reaction proceeds and whether products or reactants are favored at equilibrium.
The calculator uses the equilibrium constant formula:
Where:
Explanation: The equilibrium constant is calculated as the ratio of product concentrations to reactant concentrations, with each concentration raised to the power of its stoichiometric coefficient.
Details: The equilibrium constant is fundamental in chemical thermodynamics and kinetics. It helps predict reaction direction, extent of reaction, and is essential for understanding chemical equilibria in various systems.
Tips: Enter concentrations in molarity (M). Products and reactants concentrations must be positive values, with reactants concentration greater than zero.
Q1: What does a large K value indicate?
A: A large K value (K > 1) indicates that products are favored at equilibrium, meaning the reaction proceeds substantially toward products.
Q2: What does a small K value indicate?
A: A small K value (K < 1) indicates that reactants are favored at equilibrium, meaning the reaction does not proceed far toward products.
Q3: How are concentrations expressed in the formula?
A: Concentrations are typically expressed in molarity (moles per liter, M) for solutions, or in partial pressures for gases.
Q4: Does temperature affect the equilibrium constant?
A: Yes, the equilibrium constant is temperature-dependent. Changing temperature will shift the equilibrium position and change the value of K.
Q5: What is the difference between Kc and Kp?
A: Kc uses concentrations while Kp uses partial pressures. They are related through the ideal gas law and are used for different phases of matter.