Consider the equilibrium
reaction:          2
NO₂(g) « N₂O₄(g)

      H^o(NO₂) =
33.18
kJ/mol                  
μ^o(NO₂) = 51.31 kJ/mol
           
C_p(NO₂) = 37.20 J/mol-K

     
H^o(N₂O₄) = 9.16
kJ/mol                  
μ^o(N₂O₄) = 97.89
kJ/mol           
C_p(N₂O₄) = 77.28 J/mol-K

Compute DH_rxn at 298.15 K.

Compute DG for the reaction and use it to compute K_p
and K_c at 298.15 K.

Using the heat capacities of both species, obtain an analytical
expression for DH_rxn as a function of temperature
assuming the heat capacities are independent of temperature.

Produce analytical expressions for K_p and
K_c as a function of temperature and plot both
simultaneously as ln(K) vs. 1/T in the range of 298 K to 1000 K.
Why are the plots nearly linear and justify our not using
C_p’s as functions of temperature.

One mole of NO₂(g) is placed in a 2 L constant volume
container. Use K_c to obtain analytical expressions for
the equilibrium concentrations of both species. Using a log scale,
plot these concentrations over the same temperature range as
above.