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Question

The equilibrium constant Kp for the reaction, N2(g)+O2(g)2NO(g) at 1500oC is 120. If N2 and O2 at an initial pressure of 0.25 atm each are maintained at 1500oC till equilibrium is established, calculate the partial pressure of N2,O2 and NO in the equilibrium mixture.

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Solution

The inital partial pressures are
PN2=PO2=0.25 atm
PNO=0 atm
Let us say that x atm of nitrogen reacts with x atm of oxygen to form 2x atm of NO at equilibrium.
The equilibrium partial pressures are
PN2=PO2=0.25x atm
PNO=2x atm
KP=P2NOPN2×PO2
120=(2x)2(0.25x)×(0.25x)
10.95=2x0.25x
0.25x=2x10.95
0.25x=0.18x
0.25=1.18x
x=0.21
The equilibrium partial pressures are
PN2=PO2=0.25x=0.250.21=0.04 atm

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