A sample of 100.0 g of lead(II) oxide (223.20 g/mol) is heated in air at about 750 K until it is…

A sample of $100.0\ \text{g}$ of lead(II) oxide ($223.20\ \text{g/mol}$) is heated in air at about $750\ \text{K}$ until it is all red lead: $6\text{PbO} + \text{O}_{2} \to 2\text{Pb}_{3}\text{O}_{4}$. The red lead ($685.60\ \text{g/mol}$) is then treated with hot dilute nitric acid: $\text{Pb}_{3}\text{O}_{4} + 4\text{HNO}_{3} \to 2\text{Pb}(\text{NO}_{3})_{2} + \text{PbO}_{2} + 2\text{H}_{2}\text{O}$. Use $239.20\ \text{g/mol}$ for PbO$_2$ and $331.21\ \text{g/mol}$ for lead(II) nitrate. Find the mass of red lead, the mass of oxygen taken up, and the masses of lead(IV) oxide and lead(II) nitrate that the acid gives.