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  3. Chemistry
  4. Consider the following reaction MnO4-+8H++5e- arrow Mn+ 2+4H2O,E° =1.51V . The quantity of electricity required in Faraday, to reduce five moles of MnO4- is.

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Q. Consider the following reaction $MnO_{4}^{-}+8H^{+}+5e^{-} \rightarrow Mn^{+ 2}+4H_{2}O,E^\circ =1.51V$ .
The quantity of electricity required in Faraday, to reduce five moles of $MnO_{4}^{-}$ is______.

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Solution:

$MnO_{4}^{-}+8H^{+}+5e^{-} \rightarrow Mn^{+ 2}+4H_{2}O$
$1$ mole of $MnO_{4}^{-}$ require $5$ Faraday charge
$5$ moles of $MnO_{4}^{-}$ will require $25$ Faraday charge.