1. What is the Gibbs Free Energy Equation?

The Gibbs Free Energy equation (ΔG = ΔH - TΔS) is a fundamental thermodynamic equation that predicts the spontaneity of chemical reactions. A negative ΔG indicates a spontaneous reaction, while a positive ΔG indicates a non-spontaneous reaction.

2. How Does the Calculator Work?

The calculator uses the Gibbs Free Energy equation:

Where:

• \( \Delta G \) — Gibbs Free Energy change (kJ)
• \( \Delta H \) — Enthalpy change (kJ)
• \( T \) — Temperature (K)
• \( \Delta S \) — Entropy change (J/K)

Explanation: The equation combines enthalpy and entropy changes at a given temperature to determine whether a process will occur spontaneously.

3. Importance of ΔG Calculation

Details: Gibbs Free Energy is crucial for predicting reaction spontaneity, determining equilibrium constants, and understanding thermodynamic feasibility of chemical and biological processes.

4. Using the Calculator

Tips: Enter enthalpy change in kJ, temperature in Kelvin, and entropy change in J/K. Ensure temperature is greater than 0 K for valid calculations.

5. Frequently Asked Questions (FAQ)

Q1: What does a negative ΔG value mean?
A: A negative ΔG indicates that the reaction is thermodynamically favorable and will occur spontaneously under the given conditions.

Q2: What are typical units for thermodynamic calculations?
A: ΔH is typically in kJ/mol, ΔS in J/mol·K, and T in Kelvin. Ensure unit consistency in your calculations.

Q3: How does temperature affect ΔG?
A: Temperature can significantly influence ΔG, particularly for reactions with large entropy changes. The -TΔS term becomes more significant at higher temperatures.

Q4: Can ΔG predict reaction rates?
A: No, ΔG indicates thermodynamic spontaneity but does not provide information about reaction kinetics or speed.

Q5: What is the relationship between ΔG and equilibrium constant?
A: ΔG = -RT lnK, where R is the gas constant and K is the equilibrium constant. This relationship connects thermodynamics with chemical equilibrium.