mole of a N2O4(g)  is kept in a container under 1.0 atmospheric pressure and 27°C. It is heated to 327°C. As a result, 20% of N2O4(g)  by mass decomposed to NO2(g) The resultant pressure (atm) is

nitial temperature                              =27+273=300K.Final temperature  =327+273=600K.                            P1=1atm;P2=?According to pressure, temperature law:              P1T1=P2T2          or               1atm300K=P2600KThus,               P2=600300=2atmLet α  be the degree of decomposition of N2O4(g) to⋅ NO2(g) as :                    N2O4(g)  ⇌  2NO2(g)   2-2α           2(2α)                     Total pressure  = 2−2α+4α=  2+2αBut                          α=20100=0.2 (given)      ∴   The resultant pressure   =2+(2×0.2)=2+0.4=2.4atm