Question

Consider the following equilibrium:

2NO2g N2O4g   ΔG=−5.4kJ

Now suppose a reaction vessel is filled with 7.88atmof dinitrogen tetroxide N2O4 at 1.°C

Answer the following questions about this system:

Under these conditions, will the pressure of N2O4 tend to rise or fall? rise fall Is it possible to reverse this tendency by adding NO2 ? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2 ? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2 ? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. atm

Answer 1

Answer: the pressure of you will foll, since the reaction is having Keg of infinite Because there is no Reactonts uitially, huile the reaction will shift in Backward direction which will lead to you pressure to fall. ② Yes, it is possible to Reverse the Reaction By Addling No ③ Yes. 4 Delta Ga-RT ln (K) -5400 = 8.314 x (684+ 273) x ln(K) In(K) = 0.67869 1 k= (^(0.67869) = 1.971 = [N₂04] / [No, ]^2 [No,]^2 = 3.59/1.971 = 1.821 [no] = 1.349 atm Hence the Minimum pressure Required will be 13 atm.