How to Calculate Keq

Equilibrium Constant Formula:

\[ K_{eq} = \frac{\prod [Products]^{stoich}}{\prod [Reactants]^{stoich}} \]

Products Concentrations (comma separated):

mol/L

Products Stoichiometry (comma separated):

Reactants Concentrations (comma separated):

mol/L

Reactants Stoichiometry (comma separated):

Equilibrium Constant (K_eq):

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1. What is the Equilibrium Constant?

The equilibrium constant (K_eq) quantifies the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient in the balanced chemical equation.

2. How Does the Calculator Work?

The calculator uses the equilibrium constant formula:

\[ K_{eq} = \frac{\prod [Products]^{stoich}}{\prod [Reactants]^{stoich}} \]

Where:

\( [Products] \) — Equilibrium concentrations of products (mol/L)
\( [Reactants] \) — Equilibrium concentrations of reactants (mol/L)
\( stoich \) — Stoichiometric coefficients from balanced equation
\( \prod \) — Product notation (multiplication of all terms)

Explanation: The equilibrium constant expresses the position of equilibrium - values greater than 1 favor products, values less than 1 favor reactants.

3. Importance of Keq Calculation

Details: The equilibrium constant is fundamental in chemical thermodynamics, predicting reaction direction, extent of reaction, and is used in various chemical engineering and industrial processes.

4. Using the Calculator

Tips: Enter concentrations in mol/L and stoichiometric coefficients as integers. Separate multiple values with commas. Ensure concentrations are at equilibrium conditions.

5. Frequently Asked Questions (FAQ)

Q1: What does a large Keq value indicate?
A: A large Keq (>1) indicates the reaction favors product formation at equilibrium, with products predominating over reactants.

Q2: What does a small Keq value indicate?
A: A small Keq (<1) indicates the reaction favors reactants at equilibrium, with reactants predominating over products.

Q3: Can Keq be negative?
A: No, Keq is always positive since concentrations are always positive values raised to positive powers.

Q4: How does temperature affect Keq?
A: Keq is temperature-dependent. For exothermic reactions, Keq decreases with increasing temperature; for endothermic reactions, Keq increases with temperature.

Q5: What's the difference between Kc and Kp?
A: Kc uses concentrations (mol/L) while Kp uses partial pressures (atm). They're related through the ideal gas law for gaseous reactions.