Equilibrium Constant Expression Calculator

Equilibrium Constant Expression:

\[ K = \frac{[\text{Products}]^{\text{coeff}}}{[\text{Reactants}]^{\text{coeff}}} \]

Equilibrium Constant (K):

Unit Converter ▲

Unit Converter ▼

From:	To:

1. What is the Equilibrium Constant Expression?

The equilibrium constant expression (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their stoichiometric coefficients. It provides valuable information about the position of equilibrium in a chemical reaction.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant expression:

\[ K = \frac{[\text{Products}]^{\text{coeff}}}{[\text{Reactants}]^{\text{coeff}}} \]

Where:

\( [\text{Products}] \) — Concentration of products in moles per liter (M)
\( [\text{Reactants}] \) — Concentration of reactants in moles per liter (M)
\( \text{coeff} \) — Stoichiometric coefficient (unitless)

Explanation: The equation calculates the equilibrium constant by taking the ratio of product concentration to reactant concentration, both raised to their respective stoichiometric powers.

3. Importance of Equilibrium Constant Calculation

Details: Calculating equilibrium constants is crucial for predicting the direction of chemical reactions, understanding reaction thermodynamics, and determining the extent to which reactions proceed under given conditions.

4. Using the Calculator

Tips: Enter product concentration in M, reactant concentration in M, and stoichiometric coefficient (unitless). All values must be valid (concentrations ≥ 0, coefficient > 0, reactant concentration > 0).

5. Frequently Asked Questions (FAQ)

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

Q2: How does temperature affect the equilibrium constant?
A: The equilibrium constant is temperature-dependent. For endothermic reactions, K increases with temperature; for exothermic reactions, K decreases with temperature.

Q3: Can equilibrium constant be calculated for gaseous reactions?
A: Yes, but typically using partial pressures (Kp) rather than concentrations (Kc), unless specified otherwise.

Q4: What are the units of equilibrium constant?
A: The units depend on the specific reaction stoichiometry. For this simplified calculation, we assume appropriate units based on the coefficients.

Q5: When is this calculation most accurate?
A: This calculation is most accurate for ideal solutions at equilibrium where activities can be approximated by concentrations.