How Is Keq Calculated

Equilibrium Constant Formula:

\[ K_{eq} = \frac{[Products]}{[Reactants]} \]

Equilibrium Constant (K_eq):

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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 formula:

\[ K_{eq} = \frac{[Products]}{[Reactants]} \]

Where:

\( K_{eq} \) — Equilibrium constant (dimensionless)
\( [Products] \) — Concentration of products at equilibrium (mol/L)
\( [Reactants] \) — Concentration of reactants at equilibrium (mol/L)

Explanation: For a general reaction aA + bB ⇌ cC + dD, the complete formula is K_eq = [C]^c[D]^d / [A]^a[B]^b. This calculator simplifies to the basic ratio for educational purposes.

3. Importance Of Keq Calculation

Details: The equilibrium constant is fundamental in chemical thermodynamics and kinetics. It predicts the direction of reactions, determines reaction yields, and helps understand how conditions affect chemical equilibria.

4. Using The Calculator

Tips: Enter concentrations in mol/L. Both values must be positive numbers. The calculator provides the basic equilibrium constant ratio for educational demonstration.

5. Frequently Asked Questions (FAQ)

Q1: What does Keq value indicate?
A: K_eq > 1 favors products, K_eq < 1 favors reactants, K_eq = 1 indicates equal concentrations at equilibrium.

Q2: Is Keq affected by temperature?
A: Yes, equilibrium constants are temperature-dependent. Changing temperature shifts the equilibrium position according to Le Chatelier's principle.

Q3: What are homogeneous and heterogeneous equilibria?
A: Homogeneous equilibria involve all species in the same phase, while heterogeneous equilibria involve species in different phases (solids have constant concentration).

Q4: How is Keq different from Kc and Kp?
A: K_eq is the general term, K_c uses concentrations, K_p uses partial pressures for gaseous reactions.

Q5: Can Keq be negative?
A: No, equilibrium constants are always positive values since they represent ratios of concentrations or partial pressures.