1. What is the Equilibrium Constant?

The equilibrium constant (K_eq) is a quantitative measure of the position of equilibrium in a chemical reaction. It represents the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

Where:

• \( K_{eq} \) — Equilibrium constant (dimensionless)
• \( [Products] \) — Concentration of products at equilibrium (M)
• \( [Reactants] \) — Concentration of reactants at equilibrium (M)

Explanation: For the simplified case where all stoichiometric coefficients are 1, K_eq equals the ratio of product concentration to reactant concentration at equilibrium.

3. Importance of K_eq Calculation

Details: The equilibrium constant is fundamental in chemical thermodynamics and kinetics. It predicts the direction of chemical reactions, determines reaction yields, and helps understand how conditions affect chemical equilibrium.

4. Using the Calculator

Tips: Enter product and reactant concentrations in molarity (M). Both values must be positive, and reactant concentration must be greater than zero for valid calculation.

5. Frequently Asked Questions (FAQ)

Q1: What does K_eq > 1 indicate?
A: K_eq > 1 indicates the reaction favors product formation at equilibrium, meaning products are more abundant than reactants.

Q2: What does K_eq < 1 indicate?
A: K_eq < 1 indicates the reaction favors reactants at equilibrium, meaning reactants are more abundant than products.

Q3: How are stoichiometric coefficients handled?
A: For reactions with coefficients other than 1, concentrations must be raised to the power of their respective coefficients in the balanced equation.

Q4: What are the units of K_eq?
A: K_eq is typically dimensionless when using concentrations, though the units depend on the specific reaction stoichiometry.

Q5: How does temperature affect K_eq?
A: Temperature changes affect K_eq according to the van't Hoff equation. For exothermic reactions, K_eq decreases with increasing temperature, while for endothermic reactions it increases.