1. What is the Equilibrium Constant?

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 indicates the extent of a chemical reaction at equilibrium.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

Where:

• \( [products] \) — Molar concentrations of products at equilibrium
• \( [reactants] \) — Molar concentrations of reactants at equilibrium
• \( coefficients \) — Stoichiometric coefficients from the balanced equation

Explanation: The equation shows that K 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 Equilibrium Constant

Details: The equilibrium constant predicts reaction direction, extent of reaction, and helps calculate equilibrium concentrations. It's temperature-dependent and crucial for understanding chemical systems.

4. Using the Calculator

Tips: Enter concentrations in molarity (M), separate multiple values with commas. Ensure coefficients match the balanced equation. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

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

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

Q3: What are the units of K?
A: K is dimensionless when the number of product and reactant moles are equal. Otherwise, it has units of (concentration)^Δn.

Q4: How does temperature affect K?
A: K changes with temperature - increases for endothermic reactions, decreases for exothermic reactions when temperature rises.

Q5: What's the difference between Kc and Kp?
A: Kc uses concentrations (mol/L), Kp uses partial pressures (atm) for gas-phase reactions.