The Engineering of Chemical Reactions, Schmidt

6) The reversible gas-phase decomposition of nitrogen tetraoxide, N204, to nitrogen dioxide, NO2, is N204 42NO2 is to be carried out at constant temperature. The feed consists of pure N204 at 340K and 2 atm. The concentration equilibrium constant at 340K is 0.1 mol/dm. Calculate the equilibrium conversion of N204 in a constant volume batch reactor. (35 marks) 7) The gas-phase reaction shown is elementary and irreversible as follows: 2A (g) 2B(g) + C(g) Pure A and a diluent I are ed in equimolar ratio into a batch re so that the initial total reactor pressure is 34 bar. The reactor has a safety valve that ruptures when the total pressure exceeds 68 bar. If the reactor is a constant-volume batch reactor which has a cycle time of 100s per cycle (without any downtime), at the end of one cycle, (a) what is the pressure of A? (b) what is the molar conversion of A? (c) what is the total pressure in the reactor? (d) would the safety valve have triggered? (25+20+15+5=65 marks) Other information R=8.314 x 10-2 L-bar/K-mol Temperature is kept at 340 K The rate constant (k) is 0.01 L/mol-s Integration table is provided. Assume ideal gas