Virtual Lab Experiments
Observe dynamic equilibrium and reversible reactions in simulated closed laboratory chambers. Manipulate thermal energy to trigger reversible hydration and thermal dissociation.
Initial state: Hydrated copper(II) sulfate crystals (CuSO₄·5H₂O) at 25°C. Solid is bright blue.
This interface provides an illustrative digital simulation. Ammonia (NH₃) is an irritant to respiratory systems and eyes, and Hydrogen Chloride (HCl) gas forms toxic, corrosive fumes in air. In real educational environments, experiments with ammonium chloride must be performed inside a certified fume cupboard under teacher supervision.
Delve into Le Chatelier's Principle and the industrial conditions of the Haber Process.
Explore Equilibrium PrinciplesDynamic Equilibrium Simulator
Observe how forward and reverse reactions proceed simultaneously in a closed container. Equilibrium is achieved when forward and reverse rates become equal and concentrations stop changing.
Rate of A converting to B. Increasing shifts equilibrium to the right.
Rate of B converting back to A. Increasing shifts equilibrium to the left.
What makes this dynamic?
- Microscopic motion never halts: Reactant particles continue colliding and forming products at the exact same frequency that products revert.
- Macroscopic constancy: Because the forward and reverse rates are equal, overall amounts of reactants and products stay invariant.
- Closed boundary condition: Neither matter nor energy escapes, making reversible dynamic balance possible.