The total pressure for a mixture of N2O4 and NO2 is 0.15 atm. If Kp = 7.1 (at 25 degree celsius), calculate the partial pressure of each gas in the mixture
2NO2(g) <---> N2O4(g)
Kp = P-N2O4 / (P-NO2)^2
Kp = 7.1
PT = N2O4 + NO2 = 0.15
assume this mixture is in equilibrium
let "x" be the partial pressure of NO2 and therefore, PT = PN2O2 + PNO2 becomes
PNO2 = x
0.15 = PN2O2 - x
that is:
PN2O4 = 0.15-x
PNO2 = x
then
Kp = P-N2O4 / (P-NO2)^2
7.1 = (0.15-x)/(x^2)
solve for x
7.1*x^2 + x -0.15 = 0
x = 0.09109
then
PN2O4 = 0.15-0.09109 = 0.05891 atm
PNO2 = 0.09109 atm
Proof:
Kp = 7.1
Kp = 0.05891 /(0.09109 ^2) = 7.09982 ; which is pretty close to 7.1
therefore, it is correct
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