Reference no: EM132675483

Thermodynamics/Equilibrium - This problem is concerned with one of the most industrially important chemical reactions in history, the synthesis of ammonia. ½ N2 (g) + 3 /2 H2 (g) ↔ NH3 (g) You need the following thermodynamic data for ammonia, all at 298 K.

?fG° = -16.45 kJ mol-1
?fH° = - 46.11 kJ mol-1
S° = 192.45 J mol-1 K-1
Cp,m = 35.06 J mol-1 K-1

a) Calculate the equilibrium constant every 50° from 300 K to 1000 K both from statistical mechanics and using thermodynamic data. Treat the gases as ideal, and state any other assumptions. Comment on any differences between the calculations.

b) Derive a general expression for the extent of reaction, assuming the initial amounts are 0.5 mol N2 and 1.5 mol H2.

c) Plot the extent of reaction as a function of temperature from 300 K to 1000 K at a total pressure of 300 bar.

d) Plot the extent of reaction as a function of pressure from 10 to 300 bar at 500 K.

e) Based on your results, comment on why the industrial synthesis of ammonia is performed under conditions of high temperature and high pressure.