Make the electrons match

Chlorate ions oxidise iron(II) ions in acid. You will use the electrons gained and lost to find how many ions react, and then the number of $\text{H}^+$ ions the equation needs.

The idea. One chlorine atom goes from $+5$ in chlorate to $-1$ in chloride, a gain of 6 electrons. One iron(II) ion loses 1 electron. The numbers of ions must make the electrons equal.

Your tasks.

1. Set total to the smallest number of electrons that both gained and lost divide into.
2. Set n_ox to the number of chlorate ions that react.
3. Set n_red to the number of iron(II) ions that react.
4. Set h_plus to the number of $\text{H}^+$ ions needed on the left, so that the charge is the same on both sides.