1. 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