A student is given two beakers in the laboratory. One beaker contains a solution that is 0.14 M in Mn3+ and 0.46 M in Mn2+, and the other beaker contains a solution that is 0.28 M in Sn²+ and 0.056 M in Snª+. A piece of platinum wire is dipped into each solution. (a) Calculate the potential of each electrode relative to a standard hydrogen electrode at 25°C. Pt|Mn3+, Mn2+: Pt|Sn4+, Sn²+: (b) Predict the chemical reaction that will occur when these two electrodes are connected and a salt bridge is used to join the two solutions together. chemPad О Help X.x"| → Greek

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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.