Which is a stronger reducing agent,$Cr^{2+}$ or $Fe^{2+}$,and why?

(N/A) The following reactions occur when $Cr^{2+}$ and $Fe^{2+}$ act as reducing agents:
$Cr^{2+} \longrightarrow Cr^{3+} + e^-$
$Fe^{2+} \longrightarrow Fe^{3+} + e^-$
The standard electrode potential value $E^\circ_{Cr^{3+}/Cr^{2+}}$ is $-0.41 \ V$,while $E^\circ_{Fe^{3+}/Fe^{2+}}$ is $+0.77 \ V$.
$A$ more negative $E^\circ$ value indicates a greater tendency to undergo oxidation.
Since the $E^\circ$ value for $Cr^{3+}/Cr^{2+}$ is negative,$Cr^{2+}$ is easily oxidized to $Cr^{3+}$.
Conversely,the positive $E^\circ$ value for $Fe^{3+}/Fe^{2+}$ indicates that $Fe^{2+}$ is not easily oxidized to $Fe^{3+}$.
Therefore,$Cr^{2+}$ is a stronger reducing agent than $Fe^{2+}$.