1. What is the Equilibrium Constant Kc?

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

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

Where:

• \( [products] \) — Equilibrium concentrations of products (mol/L)
• \( [reactants] \) — Equilibrium concentrations of reactants (mol/L)
• \( coefficients \) — Stoichiometric coefficients from balanced equation

Explanation: The equation shows the ratio of product concentrations to reactant concentrations at equilibrium, with each term raised to the power of its coefficient.

3. Importance of Kc Calculation

Details: Kc helps predict reaction direction, extent of reaction, and equilibrium positions. It's fundamental in chemical equilibrium studies and industrial process optimization.

4. Using the Calculator

Tips: Enter concentrations in mol/L and coefficients as whole numbers. Separate multiple values with commas. Pure solids and liquids are not included in Kc expressions.

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 changes with temperature. Endothermic reactions increase Kc with temperature, while exothermic reactions decrease Kc.

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

Q4: How is Kc different from Kp?
A: Kc uses concentrations while Kp uses partial pressures for gas-phase reactions.

Q5: When should Kc not be used?
A: For reactions involving pure solids or liquids (their activities are 1 and don't appear in Kc expression).