For the equilibrium ,2SO3(g)⇌2SO2(g)+O2(g); the partial pressure of SO3, SO2 and O2 gases at 650K are respectively 0.2bar,0.6bar and 0.4bar. If the moles of both oxides of sulphur are so adjusted as equal, what will be the partial pressure of O2?
A
4.4
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B
0.44
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C
3.6
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D
1.12
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Solution
The correct option is D3.6 2SO3⇌2SO2+O2
Kp=[SO2]2[O2][SO3]2=(0.6)2(0.4)(0.2)2=3.6
If SO2 and SO3 are made equal,
3.6=[SO2]2[SO3]2×[O2]⇒[O2]=3.6
Because moles of SO2&SO3 are equal, PSO2,&PSO3 came each other