Final answer:
Balancing the skeletal equation of Fe + PbO₂ → Fe₂O₃ + Pb²+ under acidic conditions requires following a systematic redox balancing method by assigning oxidation numbers, balancing mass and charge with appropriate coefficients, and finalizing the equation with the lowest whole numbers.
Step-by-step explanation:
To balance the skeletal equation Fe + PbO₂ → Fe₂O₃ + Pb²+ under acidic conditions, we must follow the method of balancing redox reactions, which involves balancing the changes in oxidation states and ensuring both mass and charge are balanced.
First, assign oxidation numbers and identify the changes in oxidation states for the atoms involved. In this case, we identify that iron (Fe) is oxidizing and that lead dioxide (PbO₂) is being reduced.
Next, balance the atoms that change oxidation state (redox couple), then balance the oxygen by adding water (H₂O) molecules, and finally balance the hydrogen by adding hydrogen ions (H+).
Lastly, ensure the charge is balanced by adding electrons (e−), which are necessary for the redox reaction to occur. The final step is to ensure that the coefficients are the lowest possible whole numbers that result in the same number of atoms of each element on both sides of the equation, as well as a balanced overall charge.
However, without knowing the exact oxidation states or the full balanced equation, we cannot provide the exact coefficients.