Equilibrium Constant Calculator

Equilibrium Constant Formula:

\[ K = \frac{[products]^{coefficients}}{[reactants]^{coefficients}} \]

Products Concentrations (M):

comma separated

Products Coefficients:

comma separated

Reactants Concentrations (M):

comma separated

Reactants Coefficients:

comma separated

Equilibrium Constant (K):

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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:

\[ K = \frac{[products]^{coefficients}}{[reactants]^{coefficients}} \]

Where:

\( [products] \) — Concentrations of products at equilibrium (M)
\( coefficients \) — Stoichiometric coefficients of products
\( [reactants] \) — Concentrations of reactants at equilibrium (M)
\( coefficients \) — Stoichiometric coefficients of reactants

Explanation: The equilibrium constant is calculated by multiplying the equilibrium concentrations of the products, each raised to the power of their stoichiometric coefficient, and dividing by the same calculation for the reactants.

3. Importance of Equilibrium Constant

Details: The equilibrium constant is crucial for predicting the direction of a reaction, calculating equilibrium concentrations, and understanding how conditions affect chemical equilibrium (Le Chatelier's principle).

4. Using the Calculator

Tips: Enter concentrations in molarity (M) as comma-separated values. Make sure the number of coefficients matches the number of concentrations for both products and reactants.

5. Frequently Asked Questions (FAQ)

Q1: What does the value of K tell us?
A: K > 1 favors products, K < 1 favors reactants, and K ≈ 1 indicates significant amounts of both.

Q2: What's the difference between Kc and Kp?
A: Kc uses concentrations (M), while Kp uses partial pressures (atm) for gas-phase reactions.

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

Q4: What units does K have?
A: K is technically unitless, though the calculation may involve units that cancel out.

Q5: When is K undefined?
A: When any reactant concentration is zero (division by zero), or when all product concentrations are zero.