A fuel gas mixture of 10500 lbmol/hr 35 mol% ethane, 25 mol% propane, and the balance butane is fed to a combustion reactor with 12% excess air. In this reactor there is complete combustion only (no CO). There are fractional conversions of 82, 73, and 69% for ethane, propane, and butane, respectively. (a) Draw a PFD of the process. (b) Write down all relevant balanced equations. (c) Calculate the molar flowrate of incoming air.

1. An industrial burner has been developed that will burn a gaseous mixture of 90% methane and 10% hydrogen by volume. The system is a constant flow process with the air and fuel entering the combustion zone at 25°C and 1 atmosphere (101.3 kPa). 1.What is the dew point temperature in the exhaust system if the pressure is assumed to be 1 atmosphere? 2. An analysis of the combustion products indicates that 10% of each kmol of CO2 produced dissociates to CO and O2 (CO2 CO + 202). Write the complete reaction scheme including the dissociated products per kmol of fuel burnedand Determine the equilibrium constant (Kp) for the dissociation of CO2 within this combustion process.

A fuel gas mixture of 10500 lbmol/hr 35 mol% ethane, 25 mol% propane, and thebalance butane is fed to a combustion reactor with 12% excess air. In this reactor there iscomplete combustion only (no CO). There are fractional conversions of 82, 73, and 69% forethane, propane, and butane, respectively. (a) Draw a PFD of the process.(b) Write down all relevant balanced equations.(c) Calculate the molar flowrate of incoming air.(d) Calculate the molar flowrate of the stack gas, along with component flowrates.(e) Calculate the dry basis composition of the stack gas.(f) Calculate the wet basis composition of the stack gas.

Exercise 7.2.1: Heat from a generic reaction. A balance stoichiometric reaction 2D + 0.5E 3.8F with Ah-(100°C, 1 atm) = -48 kJ/mol. (a) If 62 mol/s of component F are produced at 100°C and 1 atm, how much heat (kW) is produced by the reaction?

Please include your diagram, mass balances, and full work. Thank you.

The heat of combustion of undecane is - 7430.9 kJ/mol. Use this value to find the heat of formation of undecane. (You may also need to use the following tabulated thermochemical data. Enter an unrounded value.) Substance AH° (kJ mol-) 02 (9) CO2 (9) -393.5 H, O(1) -285.8 C; H12 (1) -173.5 C,H16 (1) -224.2 C9 H20 (1) -274.7 C11H24 (1) -327.2 kJ/mol Activate Windows

Determine the specific volume of refrigerant-134a at 2MPA and 100°C, using (a). the ideal-gas equation of state.---- (b). the Vander Waals EOS. (Calculate the Vander Waals EOS parameters using the equations and obtain the data values form the steam tables).Compare the values obtained to the experimentally determined value of 15,000 KPa.---- (c).Using the generalized compressibility chart. Determine the error involved in each case.----

A fuel of formula C,H10O, has an enthalpy of formation of -184 MJ/kmol (at 25°C) and can be assumed to have a constant heat capacity of Co = 51 kJ/kmol-K. The fuel enters the combustor at 299 K and a flowrate of 180 kg/hr, where it is combusted with 110% stoichiometric preheated air at 450 K. Complete combustion occurs, with the products exiting the combustor at 900 K. a. What is the molar mass of the fuel? Mfuel = kg/kmol. b. What is the stoichiometric mass air-to-fuel ratio for this system? AFRtoic = c. The mass flow rate of products exiting the combustor is kg/s. d. The volumetric fraction of oxygen gas in the product stream is e. The mass fraction of carbon dioxide in the product stream is kJ/kg. f. What is the Higher Heating Value of the fuel? HHV = MW. g. What is the heat removed from the combustor? Qout =

Solve only 1st Qs Hint 1) Ans( S= 2918.13 kg/h,U = 2289. 49 W/m2 C)

Which one of the following reactions would produce the largest amount of heat per mole of oxygen?   A. 2O2(g) + CH4(g) à CO2(g) + 2H2O(g)                 ΔH°rxn = -802 kJ   B. All reactions produce the same energy per mole of oxygen   C. O2(g) + 2Ca(s) à 2CaO(s)                                    ΔH°rxn = -635 kJ   D. 3O2(g) + 2CH3OH(l) à 2CO2(g) + 4H2O(g)        ΔH°rxn = -1280 kJ