1. What is the Equilibrium Constant?

The equilibrium constant (K_eq) is a quantitative measure of the position of equilibrium in a chemical reaction. It represents the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant equation:

Where:

• \( K_{eq} \) — Equilibrium constant (dimensionless)
• \( [Products] \) — Concentration of products (M)
• \( [Reactants] \) — Concentration of reactants (M)

Explanation: The equilibrium constant provides information about the extent of a reaction and whether products or reactants are favored at equilibrium.

3. Importance of Keq Calculation

Details: The equilibrium constant is fundamental in chemical thermodynamics and kinetics. It helps predict reaction direction, calculate equilibrium concentrations, and understand reaction spontaneity under given conditions.

4. Using the Calculator

Tips: Enter product and reactant concentrations in molarity (M). Both values must be valid (concentrations ≥ 0, reactants > 0). The calculator will compute the equilibrium constant ratio.

5. Frequently Asked Questions (FAQ)

Q1: What does a large Keq value indicate?
A: A large Keq (>>1) indicates that products are favored at equilibrium, meaning the reaction proceeds nearly to completion.

Q2: What does a small Keq value indicate?
A: A small Keq (<<1) indicates that reactants are favored at equilibrium, meaning the reaction barely proceeds.

Q3: How is Keq related to reaction quotient Q?
A: Keq is the special case of Q at equilibrium. If Q < Keq, reaction proceeds forward; if Q > Keq, reaction proceeds reverse.

Q4: Does Keq change with concentration?
A: No, Keq is constant at a given temperature. It only changes with temperature, not with initial concentrations.

Q5: What are the units of Keq?
A: Keq is dimensionless for this simplified version. In complete formulations, units depend on the reaction stoichiometry.