Consider the reaction 2NO2 (g)<——> N2 O4 (g), Assume that the gases are described by the equation of state PV/n=RT+B1(T)P+B2(T)P^2/RT, where B1(T)=b-a/RT, B2(T)=b^2, a=5.354 and 6.55 L^2 bar/mol^2, b=0.04424 and 0.05636 L/mol, Cp=6.37 + 0.0101 T – 3.405 T^2 cal/mol K and Cp=10.719 + 0.0286 T – 8.726 T^2 cal/mol K for NO2(g) and N2O4(g), respectively. Do the calculations in the following points (a-g) first for a=b=0 and then for the above nonzero values. (a) Find the change of enthalpy and chemical potential for the reaction at standard conditions. (b) Calculate f/P, where f is fugacity for both gases at 298.15 K and P=1-400 bar (plot the results). (c) Obtain the values Kp and Kc at 298.15 K. (d) Obtain delta Η for the reaction from T=298.15 to 1000 K. (e) Obtain expressions for Kp and Kc as a function of T. Plot them as a function of 1/T from 298.15 to 1000 K. (f) One mole of NO2(g) is initially placed in a sealed container having a volume equal to 2 L. Obtain an expression for the equilibrium concentration of N2O4(g) as a function of T. Make a semi-log plot of this concentration vs T from 298.15 to 1000 K. (g) For the situation in (f), obtain the mole fraction of N2O4(g) present a at equilibrium as a function of total pressure over the range P=1-400 bar. Make a plot of this mole fraction vs. P.