A 10% rich mixture of Heptane (C,H16) and air is initially at a pressure of 1 bar andtemperature of 100°C, and is polytropically compressed through a volumetric ratio of 6 to1. It is ignited and adiabatic combustion proceeds at constant volume. The maximumtemperature reached is 2627°C and at this temperature the equilibrium constants arePH₂OPCO= 6.72PCO₂PH₂P²coPo₂= 0.054Pco2po' = 1bar is a reference pressure for the equilibrium constants. if the constituents of thegas are CO2, CO, H₂O, H₂, O2 and N₂:(a) Calcuate the reaction equation without dissociation(b) Calculate the equilibrium product composition.(c) Verify that approximately 30.2 % of the carbon has burned incompletely.Notes:the number of moles is not conserved in this reaction!You may use any method to solve the (nonlinear) equations you derive.

Now, we can calculate the equilibrium composition of CO2, CO, H2O, H2, O2, and N2 using the ideal…

Answered: A 10% rich mixture of Heptane (C,H16)…

Elements Of Electromagnetics

7th Edition

ISBN:9780190698614

Author:Sadiku, Matthew N. O.

Publisher:Sadiku, Matthew N. O.

ChapterMA: Math Assessment

Section: Chapter Questions

Problem 1.1MA

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H.W.3.5 Propylene (C3H6) is burned with 50 percent excess air during a combustion process. Assuming complete combustion and a total pressure of 105 kPa, determine (a) the air-fuel ratio and (b) the temperature at which the water vapor in the products will start condensing (c) the product analysis based on volume and mass.
Liquid propane (C3H8) enters a combustion chamber at 25°C at a rate of 0.07 kg/min where it is mixed and burned with 40 percent excess air that enters the combustion chamber at 7°C. An analysis of the combustion gases reveals that all the hydrogen in the fuel burns to H,0 but only 75 percent of the carbon burns to CO, with the remaining 25 percent forming CO. determine (a) the balanced equation for actual combustion process and (b) the mass flow rate of air.
Using Hess' Law, calculate for the heat of combustion of a 1.5 liter propene (C3H6) at 14.5 psi and 80.6°F that is completely burned in air. Assume that all the water produced during the reaction is in liquid state. The standard enthalpy of formation of propene, C3H6 is +20.6 kJ/mol. The heats of formation of CO₂(g) and H₂O(l) are -394 kJ/mol and -285.8 kJ/, respectively.
Liquid propane (C 3 H 8 ) enters a combustion chamber at 25 °C at a rate of 0.05 kg/min where it is mixed and burned with theoretical air that enters the combustion chamber at 7 °C. an analysis of combustion gases reveals that all the hydrogen in the fuel burns to H 2 O but only but only 90% of carbon burn to CO 2 with the remaining 10% forming Co if the exit temperature of combustion gases is 1500 K (a) the mass flow rate of air and (b) the rate of heat transfer from the combustion chamber
A gaseous fuel with 80% butane, 15% nitrogen and 5% oxygen (on a mole basis) is burned to completion with 120 percent theoretical air that enters the combustion chamber at 30°C and 100 kPa. Determine the volume flow rate of air required to burn fuel at a rate of 2 kg/min.
Determine the adiabatic flame temperature (K) for a mixture of methane and 200% theoretical air that reacts completely in a steady-flow process at 1 atm. The methane and air enter the reaction at 298 K.
One Kmol of C8H18 is burned with 100% air containing 25 Kmol of O2. Determine the air-fuel ratio for this combustion process.
One mole of C3H8, is burned with an unknown amount of air during a combustion process. An analysis of the combustion products shows that the combustion is complete and there 3 moles of free O2, in the products. Determine; - a. the actual air-fuel ration b. the equivalence ratio c. the percentage of theoretical air used during this process.
Methanol (CH3OH) is burned with 50% excess air. Write the balanced reaction equations for complete and actual combustion, and then determine (a) the actual air-to-fuel ratio, and (b) the enthalpy of the complete combustion of Methanol at 25°C and 1 atm assuming H₂O in the products is in the liquid form. N₁ hc=Hp-HR=Nphp-ENRIR TABLE 32 Standard enthalpies of formation Species State! 0₁ Gas Gav Ga Gas Gas Gas H₁ C. Co, но 1,0 CO Useful relations: Mair 123 ful C,H, CH,OH CH,OH Liqind Gas Gas Gas Gas Liquid Gas Liquid AF C₂B₁ сн.. At 298.15 K (25 C) and 1 aus Ah,, MJ/kmol 0 0 0 0 -393.52 241.83 285.84 110.54 -74.87 -101.85 -201.17 238.58 208.45 249.35
5) Determine the adiabatic flame temperature for constant-pressure combustion of a propane-air mixture at an equivalence ratio of 0.8. Assume the reactants at 298 K, no dissociation of the products, and constant specific heats evaluated at 2000 K.
Q1. Propane (C3H8) gas enters a steady-flow adiabatic combustion chamber at 25°℃ and 1 atm. It is burned with 300 percent excess air that also enters at 25°C and 1 atm. Assuming complete combustion, determine (a) the temperature of the products, (b) the entropy generation, and (c) the reversible work and exergy destruction. Assume that To = 298 K and the products leave the combustion chamber at 1 atm pressure.
A piston-cylinder arrangement initially contains 0.002 kmol of H, and 0.01 kmol of O, at 298 K and l atm. The mixture is ignited and burns adiabatically at constant pressure. Determine the final temperature assum- ing the products contain only H20 and the excess reactant. Also deter- mine the work done during the process. Sketch the process on H-T and P-V coordinates.

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