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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Determine the enthalphy of combustion of methane at 25 deg Centigrade and 1 atm, using enthalphy - of - formation data from Table A - 26. Assume the water in the products is in liquid form.
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.
(B) A mixture of CH,s and air having a fuel air ratio of 0.05 by weight is burnt in a spark ignition engine at consteat-veleme without any heat loss. The pressure and temperature of charge at the end of compression when ignition starts are 10 bar and 285 °C respectively. Calculate the pressure and temperature at the end of combustion. Assume constant specific heats and no dissociation. Values of C C,His=0,356; O, 0155: N2 =0,176; HO =0.36; co-0.158 KJ/kg K and the lower heating value of fuel=10560 kJ/kg. lo 18°
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.
Liquid octane at 25°C and 0,1MPA is burned in 96% theoretical air at 25°C. The exit temperature is 600K. How much energy is emitted to the environment? (4.19x10°kJ/kmol)
One Kmol of C8H18 is burned with 100% air containing 25 Kmol of O2. Determine the air-fuel ratio for this combustion process.
Liquid octane is burned completely with 75% excess air. Determine the air-fuel ratio for this combustion process.
Q1) A constant volume tank contain 1 mole ofC7H14 and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C7H14is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take dalta Ho = -47800 kJ/kg).

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