How many moles of $\mathrm{KMnO}_4$ are required to oxidise 1 mole of oxalic acid in acidic medium?

Ozone is quantitatively determined by bubbling it through an excess of acidic potassium iodide solution, which liberates iodine. The liberated iodine is then titrated with sodium thiosulphate solution.

If 25.0 mL of the iodine-containing solution required 20.0 mL of 0.01 M sodium thiosulphate for complete titration, calculate the number of moles of ozone that reacted.

For the given redox reaction, what will be the sum of $x, y, m$ and $n$ ?

$$\begin{aligned} x \mathrm{MnO}_4^{-}+y \mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4+z \mathrm{H}^{+} \longrightarrow m \mathrm{Mn}^{2+} + & n \mathrm{CO}_2+p \mathrm{H}_2 \mathrm{O} \end{aligned}$$

How many moles of potassium dichromate oxidises 1 mole of ferrous oxalate in acidic medium?