5. Consider a voltaic cell involving lead (II) and gold (III). Draw the galvanic cell and include the following information:

a. Identify and label the anode and the cathode.

b. Write balanced half-cell reactions for the reaction at the anode and cathode.

c. Indicate on the wire the direction in which the electrons flow.

d. Indicate which way cations from the salt bridge move.

e. Calculate the potential of the standard cell.

For a voltaic cell involving lead and gold, the anode and cathode are identified, with half-cell reactions provided. The overall reaction and standard cell notation are presented, along with details on electron flow and cation movement.

Explanation:

Half-cell reactions:
Anode: Pb(s) - 2e⁻ → Pb²⁺(aq)
Cathode: Au³⁺(aq) + 3e⁻ → Au(s)
Overall reaction:
Pb(s) + 2Au³⁺(aq) → Pb²⁺(aq) + 2Au(s)
Standard cell notation: Pb(s) | Pb²⁺(aq) || Au³⁺(aq) | Au(s)
Direction of electron flow: From anode to cathode on the wire
Cations in salt bridge: Cations move towards the cathode
Cell potential calculation: Use standard reduction potentials to calculate cell potential

Learn more about Galvanic cells and redox reactions here:

https://brainly.com/question/37147148