13.8g of N2O4 was placed in a 1L reaction vessel at 400K and allowed attain equibrium N2O4(g)⇌2NO2(g)
The total pressure at equilibrium was found to be 9.15 bar. Calculate Kc,Kp and partial pressure at equilibrium.
pressure of N2O4 at 400k
P=nRTV=0.15×0.0821×4001=4.9bar≈5
N2O4⟶2NO2
5−x 2x (at equilibrium)
Total pressure = 5+x=9.15bar or x=4.15bar
So Kp=(PNO2)2PN2O4=(2×4.15)2(0.85)2=95.34
Now, Kc=KpRTΔng=95.34×0.0821×4001=3130.96