One mole of N_2O_(4(g)) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K to decompose to NO_(2(g)). If the resultant pressure at equilibrium is 2.4 atm, then which is correct?

One mole of N_2O_(4(g)) at 300 K is kept in a closed container under o

1.	One mole of N_2O_(4(g)) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K to decompose to NO_(2(g)). If the resultant pressure at equilibrium is 2.4 atm, then which is correct?
Answer» % DISSOCIATION = 20% pressure of `NO_2` at equilibrium = 0.8 atm pressure of `N_2O_4` at equilibrium =1.2 atm `K_p = 0.4` atm Solution :`underset(1-ALPHA)underset(1)(N_(2)O_(4)) HARR underset(2alpha)underset(0)(2NO_(2))` Total no. of moles at equlibrium = `1+alpha` from Ideal gas equation `(P_(1))/(P_(2))=(n_(1)T_(1))/(n _(2)T_(2)), underset("equlibrium")underset("before")((P_(1))/(n_(1)T_(1)))=underset("equlibrium")underset("after")((P_(2))/(n_(2)T_(2)))` `(1)/(1 xx 300)=(2.4)/((1+alpha)600) implies alpha=0.2 implies %alpha = 20%` `P_(NO_(2))=(2alpha)/(1+alpha)`, Total pressure = 0.8 `K_(P)=(P_(NO2)^(2))/(P_(N_(2)O_(4)))=0.4` atm