A chemist assembles the following electrochemical cell. One side of the cell contains a zinc electrode immersed in aqueous zinc nitrate solution. The other side of the cell contains an iron electrode immersed in aqueous iron(II) nitrate solution. In this reaction, zinc is the anode and iron is the cathode. Write equations showing the half-reactions that take place at each electrode. Include phase symbols. Na+ NO3 Salt bridge Zn Fe aq. Zn(NO3)2 aq. Fe(NO3)2 anode half-reaction: cathode half-reaction:

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.