Answer:
[tex]m_{MnO_2}=21.2gMnO_2[/tex]
Explanation:
Hello,
In this case, given the balanced reaction:
[tex]2MnO_4^-+2Mn(OH)_2\rightarrow 4MnO_2+2OH^-+H_2O[/tex]
We can see a 2:4 mole ration between permanganate ion (118.9 g/mol) and manganese (IV) oxide (86.9 g/mol), that is why the resulting mas of this last one turns out:
[tex]m_{MnO_2}=14.5gMnO_4^-*\frac{1molMnO_4^-}{118.9gMnO_4^-}*\frac{4MnO_2}{2molMnO_4^-} *\frac{86.9gMnO_2}{1molMnO_2} \\\\m_{MnO_2}=21.2gMnO_2[/tex]
Best regards.
