Activation energy in chemical reactions

Référence de la vidéo 12081389
Activation energy in chemical reactions. Animation showing the importance of bond energies and activation energies in a chemical reaction. This is an example of the collision theory of chemical reactions. The animation shows the reaction between the diatomic gas hydrogen (H2, grey) and the diatomic gas chlorine (Cl2, green) to form molecules of hydrogen chloride (HCl). Labels added to the animation highlight the reactants and product. The breaking and formation of the molecular bonds is also shown, with two molecules of hydrogen chloride forming from the reaction between a molecule of hydrogen and a molecule of chlorine. The second stage of the animation (from 00:30) zooms in to show the bond energy of 432 kilojoules per mole (kJ/mol) for a hydrogen molecule and the bond energy of 240 kJ/mol for a chlorine molecule. These bond energies combined are the activation energy of 672 kJ/mol for this reaction. The animation then shows a collision with an energy below the activation energy, and hence no reaction occurring. The animation then shows ultraviolet light (UV photons, purple) raising the energy of the gas molecules. This raises the collision energy above the activation energy, and the reaction is shown taking place. The animation then shows a bond energy of 428 kJ/mol for a hydrogen chloride molecule. The final 30 seconds of the animation shows the reaction as a graph of energy against time, with the activation energy labelled.
Licence : Droits gérés
Crédit : Science Photo Library / RHYS LEWIS, AHS, DECD, UNISA
Model Release : Non requis
Durée : 02:07 Minutes
Aspect ratio : 16/9
Restrictions : -

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