Equilibrium Constant Calculator

Equilibrium Constant Formula:

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

Products Concentration (M):

Products Coefficient:

Reactants Concentration (M):

Reactants Coefficient:

Equilibrium Constant (K):

Unit Converter ▲

Unit Converter ▼

From:	To:

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 to which a reaction proceeds before reaching equilibrium.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

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

Where:

\( K \) — Equilibrium constant (unitless)
\( [\text{Products}] \) — Concentration of products at equilibrium (M)
\( [\text{Reactants}] \) — Concentration of reactants at equilibrium (M)
\( \text{coefficients} \) — Stoichiometric coefficients from the balanced equation

Explanation: The equation shows that K is the ratio of product concentrations to reactant concentrations, each raised to the power of their coefficients in the balanced equation.

3. Importance of Equilibrium Constant

Details: The equilibrium constant is crucial for predicting reaction direction, understanding reaction extent, and calculating equilibrium concentrations. It's temperature-dependent and provides insight into the thermodynamic favorability of a reaction.

4. Using the Calculator

Tips: Enter concentrations in molarity (M). For reactions with multiple products/reactants, multiply their concentrations (raised to their coefficients) before entering. Reactant concentration must be > 0.

5. Frequently Asked Questions (FAQ)

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

Q2: What does a small K value indicate?
A: A small K (<<1) indicates the reaction favors reactants at equilibrium.

Q3: How does temperature affect K?
A: K changes with temperature; endothermic reactions increase K with temperature, while exothermic reactions decrease K with temperature.

Q4: What's the difference between Kc and Kp?
A: Kc uses concentrations (M), while Kp uses partial pressures (atm) for gas-phase reactions.

Q5: How do coefficients affect K?
A: Coefficients become exponents in the equilibrium expression. Changing coefficients squares K (if coefficients are doubled).