# 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.

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