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Question

1000L of air at STP was dissolved in water and required 2.5×105 moles of KMnO4 for complete reaction of SO2 at pollutants. Thus, SO2 content in air is :

A
1.4ppm
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B
14ppm
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C
2.8ppm
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D
6.25ppm
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Solution

The correct option is A 1.4ppm
Given:
1000L of air is dissolved at Standard Temperature Pressure into Water and then requires 2.5 x 105 moles of KMnO4 for complete reaction of SO2 which is dissolved in Water.

Solution:
Eqn 1:
SO2 + H2O H2SO3
Eqn2:
2MnO4+2H2SO35H2SO4+2Mn2+
It implies 2 moles of MnO4 requires 5 moles of SO2.
Therefore, 2.5 x 103 moles of KMnO4 requires = 52 x 2.5 x 103 moles of SO2 = 6.25 x 103 moles

At STP, 6.25 x 103 moles = 6.25 x 22.4 x 103 =1.4 x 103L

In 1000L, 1.41000 x 103 = 1.4 ppm.

So, the Correct option : A

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