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Question

One mole of SO3 was placed in a two litre vessel at a certain temperature. The following equilibrium was established in the vessel :
2SO3(g)2SO2(g)+O2(g)
The equilibrium mixture reacted with 0.2 mole KMnO4 in acidic medium. Hence, Kc is :

A
0.50
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B
0.25
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C
0.125
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D
None of these
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Solution

The correct option is D 0.125
2 moles of KMnO4 in acidic medium oxidize 5 moles of SO2
0.2 moles of KMnO4 in acidic medium oxidize 0.5 moles of SO2
The initial number of moles of SO3,SO2 and O2 are 1, 0 and 0 respectively.
The equilibrium number of moles of SO3,SO2 and O2 are 12x=0.5,2x=0.5 and x=0.25 respectively.
The equilibrium concentrations of SO3,SO2 and O2 are 0.52=0.25M,0.52=0.25M and 0.252=0.125M
The equilibrium constant expression is Kc=[SO2]2[O2][SO3]2=(0.25)2×0.125(0.25)2=0.125

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