N2 (g) + c2h2 (g) → 2hcn (g)
t = 298k , p = 100 bar
none of the species may be treated as ideal gases. the feed consists of stoichiometric amounts and nitrogen and acetylene with no hcn present.
a) calculate gibbs free energy using formation data. my calculated as ~4 j/mol
b) write down the appropriate expressions for the chemical potentials of the three species which participate in this reaction. my u(i) = u(i)* + rt ln (f(i)/p*) for each species, where p* is 1 bar reference state and f(i) is fugacity.
c) give an equation that expresses how the chemical potentials you obtained for part are inter-related when the reaction attains equilibrium.
d) express the mole fraction of each species in terms of the extent of reaction, ξ, and the initial moles of acetylene, n0.
e) use the equations you obtained for parts (c) and (d), generalized correlation tables, and the lewis-randall rule to calculate the equilibrium mole fraction for each species. take n0 = 1mole.