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Question

When NO and NO2 are mixed, the following equilibria are readily obtained;
2NO2N2O4 ,KP=6.8 atm1 and NO+NO2N2O3
In an experiment when NO and NO2 are mixed in the ratio of 1 : 2, the find total pressure was 5.05 atm and the partial pressure of N2O4 was 1.7 atm. Calculate the equilibrium partial pressure of NO in atmosphere.

A
3 atm
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B
2 atm
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C
4 atm
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D
1 atm
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Solution

The correct option is D 1 atm
For I equilibrium 2NO2N2O4
KP=PN2O4(PNO2)2=6.8 ....(i)
PN2O4=1.7 atm By eq.(i) PNO2=0.5 atm
The equilibria are maintained using NO and NO2 in the ratio 1 : 2
For II equilibriumNO+NO2N2O3Initial pressureP2P0Pressure at equilibrium(px)(2Px3.4)x
3.4 atm of NO2 are used for I equilibrium to have PN2O4=1.7atm
At equilibrium (P - x) 0.5 x

( PNO2 is same for both the equilibria since both reactions are at equilibrium at a time)
Total pressure at equilibrium (Given 5.05 atm)
=PNO+PNO2+PN2O3+PN2O4
=Px+0.5+x+1.7
5.05=P+2.20
5.05=P+2.20
P=2.85 atm
2×2.85x3.4=0.5
x=1.80 atm
PNO=Px
PNO=2.851.80=1.05 atm1 atm

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