Electrochemistry: describe question

Consider the following unbalanced chemical equation.

$$\ce{Pb3O4 + HCl -> PbCl2 + Cl2 + H2O}$$

In $\ce{Pb3O4}$, lead exists in two oxidation states: +2 and +4, as indicated by the Roman numerals in the name 'lead(II,IV) oxide'. Describe the redox processes occurring in this reaction in terms of electron transfer and changes in oxidation number. In your description you should:

• assign oxidation numbers to the elements in the reactants and products
• identify which species are oxidised and which are reduced
• identify the oxidising agent and the reducing agent
• explain how the changes in oxidation numbers can be used to determine the stoichiometric coefficients for the balanced equation.

Do not include a calculation of any numerical value.