1. What is the Equilibrium Constant?

The equilibrium constant (K_eq) is a fundamental concept in chemical equilibrium that describes the ratio of product concentrations to reactant concentrations at equilibrium. At equilibrium, the reaction quotient Q equals the equilibrium constant K_eq.

2. How Does the Calculator Work?

The calculator uses the fundamental relationship:

Where:

• \( K_{eq} \) — Equilibrium constant (dimensionless)
• \( Q \) — Reaction quotient at equilibrium (dimensionless)

Explanation: When a chemical reaction reaches equilibrium, the reaction quotient Q becomes equal to the equilibrium constant K_eq. This calculator simply returns the input Q value as K_eq since they are equal at equilibrium.

3. Importance of Keq Calculation

Details: The equilibrium constant is crucial for predicting the direction of chemical reactions, determining reaction yields, and understanding chemical equilibria in various systems including industrial processes and biological systems.

4. Using the Calculator

Tips: Enter the reaction quotient value measured at equilibrium. The value must be positive and greater than zero. The calculator will return the equilibrium constant value.

5. Frequently Asked Questions (FAQ)

Q1: What is the difference between Q and K_eq?
A: Q is the reaction quotient at any point in the reaction, while K_eq is the specific value of Q when the reaction reaches equilibrium.

Q2: What does the magnitude of K_eq indicate?
A: K_eq > 1 favors products, K_eq < 1 favors reactants, and K_eq = 1 indicates comparable amounts of reactants and products at equilibrium.

Q3: Can K_eq change with conditions?
A: K_eq is constant for a given reaction at a specific temperature, but changes with temperature according to the van't Hoff equation.

Q4: How is Q calculated for different reaction types?
A: For a reaction aA + bB ⇌ cC + dD, Q = [C]^c[D]^d / [A]^a[B]^b, where concentrations are at any point in the reaction.

Q5: What are the units of K_eq?
A: K_eq can be dimensionless (when using activities) or have units depending on the reaction stoichiometry when using concentrations or partial pressures.