1. What is the Equilibrium Constant Expression?

The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their stoichiometric coefficients. It's a fundamental concept in chemical equilibrium studies.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant expression:

Where:

• \( [A], [B] \) — Concentrations of reactants (mol/L)
• \( [C], [D] \) — Concentrations of products (mol/L)
• \( a, b \) — Stoichiometric coefficients of reactants
• \( c, d \) — Stoichiometric coefficients of products

Explanation: The equilibrium constant is dimensionless and provides information about the position of equilibrium.

3. Importance of Equilibrium Constant

Details: The equilibrium constant helps predict the direction of reaction, extent of reaction, and is essential for understanding chemical equilibria in industrial processes and biological systems.

4. Using the Calculator

Tips: Enter all concentrations in mol/L and their respective exponents (stoichiometric coefficients). Concentrations must be ≥0 and exponents must be positive integers.

5. Frequently Asked Questions (FAQ)

Q1: What does a large K value indicate?
A: A large K (>1) indicates the reaction favors product formation at equilibrium.

Q2: What does a small K value indicate?
A: A small K (<1) indicates the reaction favors reactant formation at equilibrium.

Q3: How does temperature affect K?
A: K is temperature-dependent. For endothermic reactions, K increases with temperature; for exothermic reactions, K decreases.

Q4: What's the difference between Kc and Kp?
A: Kc uses concentrations (mol/L) while Kp uses partial pressures (atm) for gas-phase reactions.

Q5: When is K undefined?
A: K is undefined when denominator is zero (all reactant concentrations are zero).