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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 8 mg dissolved oxygen will consume:

A
5×104 mole Mn2+
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B
2.5×104 mole Mn2+
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C
10 mole Mn2+
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D
2 mole Mn2+
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Solution

The correct option is A 5×104 mole Mn2+

1 mole of 02consumes2 moles of Mn+2

8mg consumes :-

32 g makes 1 mole of O2

1gmakes132 moles of O2

8×103 g makes 1×8×103moles of O232

=0.25×103moles

1 mole of O2 consumes 2 mole of Mn+2

0.25×103 moles will consume 2×0.25×103

=5×104 moles

Hence, option A is correct.


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