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:

• [A], [B] — Equilibrium concentrations of reactants (M)
• [C], [D] — Equilibrium concentrations of products (M)
• a, b — Stoichiometric coefficients of reactants
• c, d — Stoichiometric coefficients of products
• K — Equilibrium constant (unitless or with units depending on reaction)

3. Importance of Equilibrium Constant

Details: The equilibrium constant predicts reaction direction, extent of reaction, and how systems respond to disturbances (Le Chatelier's Principle). It's fundamental in chemical engineering, biochemistry, and environmental science.

4. Using the Calculator

Tips: Enter stoichiometric coefficients and equilibrium concentrations for reactants and products as comma-separated values. Ensure coefficients match corresponding concentrations in order.

5. Frequently Asked Questions (FAQ)

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

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

Q3: What are the units of K?
A: K is unitless when the number of product and reactant moles are equal. Otherwise, it has units of (M)^Δn where Δn is moles products - moles reactants.

Q4: How does temperature affect K?
A: K changes with temperature - endothermic reactions increase K with temperature, exothermic reactions decrease K with temperature.

Q5: What's the difference between Kc and Kp?
A: Kc uses concentrations (M), Kp uses partial pressures (atm) for gas-phase reactions. They're related by Kp = Kc(RT)^Δn.