Products formed on the reduction of KMnO4 in aqueous solution

The [Latimer diagram](https://en.m.wikipedia.org/wiki/Latimer_diagram) for $\ce{MnO^-\_4}$ is given below:


$$ \ce{MnO^{-}\_4 ->[0.56V] MnO^{2-}\_4 ->[2.26V] MnO\_2 ->[0.95V] Mn^{3+} ->[1.51V] Mn^{2+} ->[-1.18V] Mn}$$


Then I have calculated the standard reduction potential values for the convertion of $\ce{MnO^-\_4}$ to $\ce{MnO^{2-}\_4,MnO\_2,Mn^{3+},Mn^{2+}and Mn}$.   



The values are found to be :


$$ \ce{MnO^{-}\_4 ->[0.56V] MnO^{2-}\_4}$$
$$ \ce{MnO^{-}\_4 ->[1.693V] MnO\_2}$$
$$ \ce{MnO^{-}\_4 ->[1.5075V] Mn^{3+}}$$
$$ \ce{MnO^{-}\_4 ->[1.508V] Mn^{2+}}$$
$$ \ce{MnO^{-}\_4 ->[0.74V] Mn}$$


So according to the $\mathrm{SRP}$ values the feasibility for the formation of respective products follows the order:


$$ \ce{ MnO\_2 > Mn^{2+} > Mn^{3+} > Mn > MnO^{2-}\_4 } $$


So my question is which is the favourable product formed on the reduction of $\ce{KMnO4}$ in acidic solutions.  
 The values suggests that the formation of $\ce{MnO\_2}$ is preferred over others.  
 But it is not observed in experimental reactions. Most of the reaction suggests that $\ce{Mn^{2+}}$ is the favorable product.   

For example:


1. In oxidation of toulene to benzoic acid, the total redox reaction is:
$$\ce{5 C6H5CH3 + 6 KMnO4 + 9 H2SO4 -> \\5 C6H5COOH + 14 H2O + 3 K2SO4 + 6 MnSO4}$$
2. In oxidation of ferrous ions to ferric ions, that is:
$$\ce{10FeSO4 + 2KMnO4 + 8H2SO4 -> \\5Fe2(SO4)3 + 2MnSO4 + K2SO4 + 8H2O}$$


And there are many more reactions that are known to us in which formation of $\ce{Mn^{2+}}$ takes place. So why there is such disprency between experimental and observed facts. Which other factors influences here?   
 **Note:** There are some questions related to this topic but none of them has an appropriate answer to this question.


