Statement 1 : ${\mathrm{E}}^0\mathrm{for}{\mathrm{Mn}}^{3+}/{\mathrm{Mn}}^{2+}$ is more positive than ${\mathrm{Cr}}^{3+}/{\mathrm{Cr}}^{2+}.$

Statement 2 : The third ionisation energy of Mn is larger than that of Cr.

It is known that the value of $E^0$ becomes more negative down the series. As the chromium is present below in electrochemical series than $\mathrm{Mn}$, so $\mathrm{Mn}$ has more positive $E^0$ value than Cr.

$\begin{array}{l}\mathrm{Mn}\to 3{\mathrm{d}}^{5}4{\mathrm{s}}^2 ; {\mathrm{Mn}}^{2+}\to 3{\mathrm{d}}^{5}4{\mathrm{s}}^0\\ \mathrm{Cr}\to 3{\mathrm{d}}^{5}4{\mathrm{s}}^1 ; {\mathrm{Cr}}^{2+}\to 3{\mathrm{d}}^{4}4{\mathrm{s}}^0\end{array}$

For elimination of one electron from $M{n}^{2+},$ more energy is required due to its stable configuration. That is why third Ionization energy of Mn is larger than Cr.