A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) Pb2* (aq)...

  

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A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) → Pb2* (aq) + NO3 (ag) 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 PbO2l Pb2+ half-reaction has a standard reduction potential (E°) of 1.46 V and the NO37 NO half-reaction has a standard reduction potential (E°) of 0.96 V. Calculate the potential of the cell at 25 °E under the following conditions: 0.950 PNO atm 0.0500 [Pb2*] 0.0620 [NO3 ] pH 4.67 A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) → Pb2* (aq) + NO3 (ag) 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 PbO2l Pb2+ half-reaction has a standard reduction potential (E°) of 1.46 V and the NO37 NO half-reaction has a standard reduction potential (E°) of 0.96 V. Calculate the potential of the cell at 25 °E under the following conditions: 0.950 PNO atm 0.0500 [Pb2*] 0.0620 [NO3 ] pH 4.67