Delta G To K Calculator

Equilibrium Constant Equation:

\[ K = e^{-\Delta G / (R T)} \]

Equilibrium Constant (K):

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1. What Is The Delta G To K Equation?

The Delta G to K equation calculates the equilibrium constant (K) from the Gibbs free energy change (ΔG) using the relationship between thermodynamic parameters. This fundamental equation connects the spontaneity of a reaction with its equilibrium position.

2. How Does The Calculator Work?

The calculator uses the equilibrium constant equation:

\[ K = e^{-\Delta G / (R T)} \]

Where:

\( K \) — Equilibrium constant (dimensionless)
\( \Delta G \) — Gibbs free energy change (J/mol)
\( R \) — Gas constant (8.314 J/mol·K)
\( T \) — Temperature (K)
\( e \) — Euler's number (approximately 2.71828)

Explanation: The equation shows that when ΔG is negative (spontaneous reaction), K > 1, favoring products. When ΔG is positive (non-spontaneous), K < 1, favoring reactants.

3. Importance Of Equilibrium Constant Calculation

Details: Calculating the equilibrium constant from Gibbs free energy is essential for predicting reaction direction, understanding chemical equilibrium, and designing industrial processes. It provides quantitative insight into how far a reaction will proceed under given conditions.

4. Using The Calculator

Tips: Enter Gibbs free energy change in J/mol, temperature in Kelvin, and gas constant (default is 8.314 J/mol·K). Ensure temperature is positive and in absolute scale (Kelvin).

5. Frequently Asked Questions (FAQ)

Q1: What does the equilibrium constant tell us?
A: The equilibrium constant indicates the ratio of products to reactants at equilibrium. K > 1 favors products, K < 1 favors reactants, and K ≈ 1 indicates significant amounts of both.

Q2: How does temperature affect the equilibrium constant?
A: Temperature affects K through the exponential relationship. For exothermic reactions, K decreases with increasing temperature; for endothermic reactions, K increases with temperature.

Q3: What are typical units for ΔG?
A: Gibbs free energy is typically expressed in J/mol or kJ/mol. Ensure consistent units with the gas constant (8.314 J/mol·K).

Q4: Can this equation be used for any reaction?
A: This equation applies to reactions at equilibrium under standard conditions. For non-standard conditions, the relationship becomes more complex.

Q5: What is the significance of a negative ΔG?
A: A negative ΔG indicates a spontaneous reaction under standard conditions, corresponding to K > 1, meaning products are favored at equilibrium.