Galvanic cell chemistry, animation

Référence de la vidéo 11944940
Galvanic cell chemistry. Animation showing the chemistry of a galvanic cell, also called a voltaic cell. This is the principle of an electric battery, with the electrochemical reactions producing a voltage that powers a light bulb (centre towards middle of clip). The animation starts with aqueous solutions of zinc sulphate (ZnSO4) and copper sulphate (CuSO4) being poured from conical flasks into beakers to form two half-cells. Strips of solid zinc (Zn) and copper (Cu) metal act as the electrodes (anode and cathode respectively). A salt bridge (centre) soaked in sodium chloride (NaCl, table salt) is used to connect the half-cells. Metals have different reactivity, and a list of metals ordered by reactivity shows copper has a lower reactivity than zinc. A voltmeter is used to measure a voltage of 1.10 volts. The inset animations show the reactions at the surface of the metal electrodes. Zinc metal atoms give up two electrons to produce zinc ions (Zn2+) which enter solution (water molecules shown, H2O). The electrons are shown powering a light bulb and then causing copper ions (Cu2+) from solution to be deposited as copper atoms on the copper electrode. This loss of copper ions turns the solution at right negative. Electrical neutrality is maintained by the presence of the salt bridge. The animation shows sodium ions (Na+) drawn into copper sulphate solution to balance the negative charge. Similarly, in the other half-cell, the increase in zinc ions causes a rise in positive charge, balanced by chloride ions (Cl-) from the salt bridge. The salt bridge allows the reaction to continue, and the light bulb to continue drawing electrical power from the galvanic cell.
Licence : Droits gérés
Crédit : Science Photo Library / EQUINOX GRAPHICS / RHYS LEWIS, AHS, DECD, UNISA
Model Release : Non requis
Durée : 02:49 Minutes
Aspect ratio : 16/9
Restrictions : -

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