Dinitrogen tetroxide, n2o4, is in equilibrium with nitrogen dioxide, no2, according to equation 2: n2o4 (g) < -> 2 no2 (g)

(a) 2.00 g n2o4 is introduced into a 1.00 l evacuated container and its vapor allowed to come to equilibrium at 25.0 ºc, giving rise to a final total pressure of 0.653 bar. calculate keq for eq 2 at 25.0 ºc.

(b) when the temperature of the container in (a) is raised to 50.0 ºc, the total pressure increases to 0.838 bar. calculate ∆hº and ∆sº for reaction (2).

c) since reaction (2) involves breaking the n–n bond in n2o4, its ∆hº can be equated to the bond dissociation enthalpy for the n–n bond in n2o4. is this value significantly different from the typical bde of an n–n bond given in your textbook? if so, suggest a reason for the discrepancy.