Question

The quantity of electricity required to reduce 0.5 mole of MnO4– to Mn2+ is

Answer 1

Answer:

The quantity of electricity required to reduce 0.5 mole of MnO4– to Mn2+ is = 2.4 × 105 C

Explanation:

Q = 0.5 × 5 × 96500 C

= 2.4 × 105 C

Answer 2

Answer:

2.5 Faraday of electricity is required to reduce 0.5 mole of $MnO^{-}_{4}$ to $Mn^{+2}$

Explanation:

In, $MnO^{-}_{4}$ the oxidation number of Mn is +7,

Therefore,

$Mn^{+7}+5e^{-} = Mn^{+2}$

which means 5 electrons will be needed,

Therefore 5 faraday will be neede to reduce one mole of  $MnO^{-}_{4}$

so for 0.5mole,

$=0.5\times 5\\=2.5 \:F$

So, 2.5 Faraday of electricity is required to reduce 0.5 mole of $MnO^{-}_{4}$ to $Mn^{+2}$

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