1. What is the Equilibrium Constant?

The equilibrium constant (Kc) quantifies the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their stoichiometric coefficients. It indicates the extent of a chemical reaction at equilibrium.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

Where:

• \( [products] \) — Concentrations of products at equilibrium (mol/L)
• \( [reactants] \) — Concentrations of reactants at equilibrium (mol/L)
• \( coefficients \) — Stoichiometric coefficients from the balanced equation

Explanation: The equation shows that Kc is the product of the product concentrations (each raised to their coefficient) divided by the product of the reactant concentrations (each raised to their coefficient).

3. Importance of Kc Calculation

Details: Kc helps predict reaction direction, extent of reaction, and equilibrium positions. It's fundamental in chemical kinetics and thermodynamics.

4. Using the Calculator

Tips: Enter concentrations separated by commas. Ensure the number of concentrations matches the number of coefficients. Pure solids and liquids should be omitted as they have constant concentrations.

5. Frequently Asked Questions (FAQ)

Q1: What does a large Kc value indicate?
A: A large Kc (>1) means products are favored at equilibrium, while a small Kc (<1) means reactants are favored.

Q2: How does temperature affect Kc?
A: Kc is temperature-dependent. For endothermic reactions, Kc increases with temperature; for exothermic reactions, it decreases.

Q3: What units does Kc have?
A: Kc is technically unitless, but its numerical value depends on the concentration units used (typically mol/L).

Q4: When should Kp be used instead of Kc?
A: Kp (using partial pressures) is used for gas-phase reactions when concentrations aren't easily measurable.

Q5: How do catalysts affect Kc?
A: Catalysts don't affect Kc - they only speed up reaching equilibrium without changing the equilibrium position.