Question

what will be the equivalent weight
of permanganate ion in the following
I redox reactions ?
Mno4- +8H+ + 5e-
mn+2 + 4H2o​

Answer 1

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Answer 2

Equivalent weight of the permanganate ion is 31.61 g per equivalent

Explanation:

A substance's equivalent weight (oxidant or reductant) is determined by multiplying its molecular weight by the number of electrons it loses or gains during a redox reaction.

Equivalent weight = Molar mass / Number of electrons lost or gained

We know that ,

The molecular mass of Kmno4 = 158.04g

In acidic medium:

$MnO_{4} + 8H +5e^{-} - > Mn_{2} + 4h_{2} O$

n= 5

Equivalent weight = 158.04/5

= 31.61 g

In neutral medium:

$MnO_{4} + 8H +5e^{-} - > Mn_{2} + 4h_{2} O$

n=1

Equivalent weight = 158.04/1

= 158.04

In neutal medium

$MnO_{4} + 8H +5e^{-} - > Mn_{2} + 4h_{2} O$

n = 3

Equivalent weight = 158.04 /3

= 52.68 g

Ratio of equivalent mass = 3:15:5

Final answer:

Equivalent weight of the permanganate ion using redox reaction  is 31.61 g per equivalent

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