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) + NO, (ag) a) Balance the above reaction in acidic solution. b) Draw a diagram of the voltaic cell. Label the PbOz, NO, Pb2, and NO,. 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: 0.950 PNO atm 0.0500 [Pb2+] 0.0620 [NO3] M pH 4.67 A voltaic cell employs the following redox reaction: PbO2 (s) + NO (g) → Pb2* (aq) + NO, (ag) a) Balance the above reaction in acidic solution. b) Draw a diagram of the voltaic cell. Label the PbOz, NO, Pb2, and NO,. 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: 0.950 PNO atm 0.0500 [Pb2+] 0.0620 [NO3] M pH 4.67
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Related Book For
Chemistry The Central Science
ISBN: 978-0321696724
12th edition
Authors: Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward
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