N2O4 dissociates as N2O4⇌2NO2. At 55∘C and one atmosphere, % decomposition of N2O4 is 50.3%. At what P and same temperature, the equilibrium mixture will have the ratio of N2O4:NO2 as 1:8?
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Solution
N2O4(g)⇌2NO2(g) At equilibrium (1−x)2x pN2O4=(1−x)(1+x)×P;pNO2=2x(1+x)×P Kp=(2x(1+x).P)2((1−x)(1+x).P)=4x2P1−x2 Given x=0.503 and P=1
∴Kp=1.3548
CASE II: N2O4(g)⇌2NO2(g) (1−x)2x given 1−x2x=18 x=0.8 Let the new pressure be P atm Kp=4x2P1−x2=1.3548 P=0.19atm