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Question


I. 2Mn2+(aq)+4OH(aq)+O2(g)2MnO2(s)+2H2O(l)

II.MnO2(s)+2I(aq)+4H+(aq)Mn2+(aq)+I2(aq)+2H2O(l)

III. 2S2O23(aq)+I2(aq)S4O26(aq)+2I(aq)

Dissolved oxygen in water is determined by using a redox reaction. If the above equations describe the procedure then how many moles of S2O23 are equivalent to each mole of O2?

A
0.5
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B
1
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C
2
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D
4
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Solution

The correct option is D 4
Dissolved oxygen in water is given by:
(1) 2Mn+2(aq)+4OH(aq)+O2(g)MnO2( s)+2H2O
(2) MnO2(s)+2I(aq)+4H+(aq)Mn+2(aq)+I2(aq)+2H2O
(3) 2S2O23(aq)+I2 (aq) S4O26(aq)+2I
from eq (1):
1 mole of O2 gives 2 moles of MnO2
rom eq (2) :
1 mole of MnO2 gives 1 mole of I2
i.e. 1 mole of O2 gives 2 mole of I2
2 moles of S2O23 react with 1 mole of I2

So, 4 moles of S2O23 will react with 2 moles of I2
and 2 moles of I2 react with 1 mole of O2,
Therefore option: D

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