20% 4. A CH4 - N2 fuel gas mixture is burned with air (80 moi% 02 and 20%N2) in a continuous steady-state combustion reactor to yield a mixture of oxygen, nitrogen carbon monoxide, carbon dioxide, and...

Extracted text: 20% 4. A CH4 - N2 fuel gas mixture is burned with air (80 moi% 02 and 20%N2) in a continuous steady-state combustion reactor to yield a mixture of oxygen, nitrogen carbon monoxide, carbon dioxide, and water. The combustion reactions taking place are: (1) CH4 + 202 → C02 + 2H20 *complete combustion, the desired reaction (2) CH4 +02 → C0 + 2H20 *partial combustion, the side reaction 2 The outlet flue gas is flowing at a rate of 100.0 mol/min and is composed of 6.0 % CO2, 1.0% CO, 3.5% O2, 75.5% N2, and 14.0 mol% H2O. A flow chart of the process is shown icty=M below, with the following notation: CO=CO2, CO=CO, 02=0, N=N and H2O=W, Fuel gas Outlet flue gas nm1 = N3 no3 ńco2 3 = ńco 3 nw 3 = Combustion Reactor %3D Air no2 = 3 a. Calculate the molar flow rates each species in the outlet flue gas. Label on the flow chart. b. Determine the extents of reaction for complete combustion, š1), and partial combustion, Š(2). (hint: you can solve for these by writing just 2 balances)