Gibbs Free Energy
This interactive simulator explores Gibbs Free Energy in Chemistry. ΔG = ΔH − TΔS; sign vs spontaneity at constant p,T (no Q or K). Use the controls to change the scenario; watch the visualization and any graphs or readouts to connect the model with lectures, labs, and homework.
Who it's for: Suited to beginners and first exposure to the topic. Typical context: Chemistry.
Key terms
- gibbs
- free
- energy
- gibbs free energy
- chemistry
Endothermic (ΔH > 0) can still be spontaneous if TΔS is large enough; exothermic with large negative ΔS can become non-spontaneous at low T.
How it works
At **fixed temperature and pressure**, the **sign of ΔG** (for a reaction written as **products − reactants**) tells you whether the process tends to run **forward** (**ΔG < 0**) in the thermodynamic limit. **ΔG = ΔH − TΔS**: **enthalpy** and **entropy** oppose or reinforce depending on **T**. This is a **state-function** sketch — no activities, **non-standard** **ΔG** vs **Q**, or **equilibrium** **K** here.
Key equations
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