Consider a simple galvanic cell consisting of two beakers by a salt bridge.One beaker contains a solution of MNO4- in dilute sulfuric acid and has a Pt electrode.The other beaker contains a solution of Sn2+ in dilute sulfuric acid,also with a pity electrode.When the two electrodes are conected by a wire, current flows and spontaneous reaction occurs that is described by the following balanced chemical equation: 2MnO-4(aq)+5Sn2+(aq)+16H+(aq)➡2Mn2+(aq)+5Sn4+(aq) +8H2O(l) For this galvanic cell, a. Write the half-reaction that occurs at each electrode b.indicate which electrode us the cathode and which is the anode c.indicate which electrode is the positive electrode and which is the negative electrode

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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.