PbO2 + 4H+ + SO42– + 2e– → PbSO4 +2H2O

How does the oxidation number for lead (Pb) change?

1 answer

Pb goes from 4+ on the left to 2+ on the right.
PbO2. You know O is 2-, two of them makes 4- so Pb must be + in order for the comound to be zero. All compounds are zero.
On the right you know SO4^2- in PbSO4 is 2- so Pb must be 2+. You don't know how to determine oxidation states. Here is a very good site. Specifically you want to look at #2.

https://www.chemteam.info/Redox/Redox.html
Similar Questions
  1. Given:PbSO4 + 2e− Pb + SO42− E° = -0.356 V PbO2 + 4H+ + SO42− + 2e− PbSO4 + 2H2O E° = 1.685 V Determine the cell
    1. answers icon 2 answers
    1. answers icon 3 answers
  2. Find the half Reactiona) OX Pb + SO4^2- --> PbSO4 b) OX: PbO2 + SO4^2- --> PbSO4 c) OX: Pb +SO4^2- --> PbSO4 + 2 e- d) OX: Pb +
    1. answers icon 3 answers
    1. answers icon 1 answer
more similar questions