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Question

In the following gaseous phase equilibrium at constant temperature.
2SO2(g)+O2(g)2SO3(g)
The concentration of [SO2]=3.0×103M, [O2]=3.5×103 M, [SO3]=5.0×102 M. Calculate equilibrium constant.

A
Kc=7.936×104
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B
Kc=17.936×104
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C
Kc=12.936×102
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D
Kc=2.936×104
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Solution

The correct option is A Kc=7.936×104
Given, the concentration of [SO2]=3.0×103M; [O2]=3.5×103M; [SO3]=5.0×102M
For the reaction,
2SO2(g)+O2(g)2SO3(g)
Kc=[SO3]2[SO2]2[O2]
Putting all the values,
=(5×102)2(3×103)2(3.5×103)=7.936×104

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