A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) → Pb2+ (aq) + NO3− (aq)  a) Balance the above reaction in acidic solution. b) Draw a diagram of the voltaic cell. Label the PbO2, NO, Pb2+, and NO3−. Indicate the direction of electron flow and the direction of anion and cation flow from the salt bridge. c) The PbO2/ Pb2+ half-reaction has a standard reduction potential (E°) of 1.46 V and the NO3-/ NO half-reaction has a standard reduction potential (E°) of 0.96 V. Calculate the potential of the cell at 25 °C under the following conditions: PNO 0.950 atm [Pb2+] 0.0500 M [NO3−] 0.0620 M pH 4.67

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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.