Half-reactions: Au3+(aq) + 3e- Au(s) Cd2+(aq) + 2e-→ Cd(s) E: +1

Au3+ changed in to Au .The oxidation state of Au decreased from
3+ to 0 . Hence it Au3+ is reduced **

Cd changed to Cd2+ . its oxidation state increased from
zero to 2+ . Since there is an increase in oxidation state.
Cd i s undergone oxidation **

The species which undergone oxidation is reducing agent. Hence
Cd is reducing agent**

The species which undergone reduction is oxidizing agent. Hence
Au3+ is oxidizing agent **

electrons gained must be = electron lost in the overall reaction
Hence a total of 6 electrons involved. **

The species with higher reduction potential will have a strong tendency
to get reduced. This happens spontaneously. A voltaic cell
involve spontaneous reaction. here Au3+ has higher reduction
potential value ,but it undergone reduction .Hence the cell is
voltaic cell **
using these points we can answer

1)
Cd(s) is being oxidized
2)
Au3+(aq) is being reduced

3)
Cd(s) is acting as a reducing agent

4)
Au3+ is acting as a oxidizing agent

5) 6 mols of electrons are transferred

6)The reaction is a voltaic cell