What should be the reaction between lead oxide and dilute sulfuric acid? I know for a fact that dilute $\ce{H2SO4}$ is a non-oxidizing acid which makes it a reducing agent. I also know for a fact that $\ce{PbO2}$ is a strong oxidizing agent. So, I thought Redox reaction should have occurred between them, but my teacher says that no reaction occurs between the said reactants because $\ce{PbO2}$ does not react with low concentration of acid. If it were so, why does $\ce{PbO2}$ react with dilute $\ce{HCl}$. Since, both dilute $\ce{HCl}$ and dilute H2SO4 are reducing acids of low concentrations, both should be eligible for the Redox reaction.

I have tried this on the internet but all I get are reaction balancing links .JD Lee's Concise Inorganic Chemistry has nothing about this also.
YOur logic is wrong.


  I know for a fact that dilute $\ce{H2SO4}$ is a non-oxidizing acid...


sort of, but so far so good.


  ...which makes it a reducing agent.


This is where you are wrong, just because it is non-oxidizing does not make it reducing. Concentrated $\ce{H2SO4}$ is an oxidizer, diluting it does not make it less of an oxidizer, but limits the strength/mechanism.

A similar example is mixing nitroglycerin and diatomaceous earth doesn't make nitroglycerin less explosive, it just makes it harder for it to explode (dynamite).