This animation demonstrates how adding reactant concentration shifts chemical equilibrium, using the Haber process N2 + 3H2 ⇌ 2NH3 as a model. It shows the system at equilibrium, then visualizes extra N2 molecules being introduced, and traces how the forward reaction accelerates to consume the excess, producing more NH3. A closing summary reinforces Le Chatelier's principle. Useful for chemistry students learning equilibrium shifts and industrial reaction optimization.
Narrated · 16:9 · Preview before teaching · automatic layout checks do not establish subject accuracy
Create a 15-second educational 2D scientific animation explaining the effect of concentration on chemical equilibrium according to Le Chatelier’s principle. Use the Haber process: N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Scene 1 (0–4 s): Show a transparent reaction vessel containing nitrogen molecules N₂ and hydrogen molecules H₂ on the left and ammonia molecules NH₃ on the right. Show a clear reversible equilibrium arrow ⇌ between reactants and products. Display the label “Equilibrium”. Scene 2 (4–7 s): Visually add several additional N₂ molecules to the reaction vessel. Display the label “Increase in N₂ concentration”. Scene 3 (7–12 s): Show the equilibrium responding to the disturbance. Visually emphasize the forward reaction and show some of the added N₂ being consumed to form NH₃. The equilibrium should shift toward the product side. Scene 4 (12–15 s): Display the conclusion clearly: “Reactant concentration ↑ → Equilibrium shifts toward products” Add a small caption: “The system opposes the increase by consuming added N₂.” Keep the animation scientifically accurate, clean, minimal, classroom-friendly, with clear labels and no unnecessary decorative elements. Do not change the molecular identities during the animation.