Aliquid fuel has a composition (by volume) C2H6 16% and CH4 84%. It is burnedwith theoretical amount of air required for stoichiometric mixture. Calculate the molecularweight of the fuel and the fuel air ratio of the mixture. Also determine the composition(weight basis) of the product of combustion (consider that H20 does not condense).Ans:- 18.24 F/A = 0.059 ; CO₂ 15.7%; H₂O = 12% : N₂ =72.3%.,

Answered: Aliquid fuel has a composition (by…

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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Ql:- C4HS is burned in an engine with a fuel-rich air-fuel ratio. Dry analysis of the exhaust gives the following volume percents: COz 14.95%, C4HS 0.75%, CO 0%, Hz 0%, Oz 0%, with the rest being Nz. Higher heating value of this fuel is QHHV = 46.9 MJ/kg. Write the balanced chemical equation for one mole of this fuel at these conditions. Calculate: (a) Air-fuel ratio. (b) Equivalence ratio. (c) Lower heating value of the fuel. [MJ/kg] (d) The energy released when one kg of this fuel is burned in the engine with a combustion efficiency of 98%. [MJ]
C4Hs is burned in an engine with a fuel-rich air-fuel ratio. Dry analysis of the exhaust gives the following volume percents: CO2 = 14.95%, C4H8 0.75%, CO = 0%, H2 = 0%, O2 = 0%, with the rest being N2. Higher heating value of this fuel is QHHV = 46.9 MJ/kg. Write the balanced chemical equation for one mole of this fuel at these conditions. Calculate; a) Air-fuel ratio. b) Equivalence ratio. c) Lower heating value of fuel. [MJ/kg] d) Energy released when one kg of this fuel is burned in the engine with a combustion efficiency of 98%. [MJ]
Write the complete combustion reaction of fuel oil with atmospheric air. The fuel has the following mass composition: C = 85.5%, H = 10.6% and S = 3.9%. Calculate the content of CO₂ and SO₂ in volume, on a dry basis.
C,Hs is burned in an engine with a fuel-rich air-fuel ratio. Dry analysis of the exhaust gives the following volume percents: CO, 14.95%, C,H, 0.75%, CO 0%. H = 0%, O, 0%, with the rest being N. Higher heating value of this fuel is Quav 46.9 MJ/kg. Write the balanced chemical equation for one mole of this fuel at these conditions Calculate: (a) Air-fuel ratio. (b) Equivalence ratio. (c) Lower heating value of fuel. [MJ/kg] (d) Energy released when one kg of this fuel is burned in the engine with a combustion efficiency of 98%. [MJ]
Fuel and Combination Problem. Please solve ellaborately and include the Units. Your work will be appreciated much Dear.
In an engine test the dry volumetric analysis of the products was CO2 0.0527, O2 0.1338 and N2 0.8135. Assume the fuel is a pure hydrocarbon and that it is completely burnt. Write the complete balance chemical equation on volume basis. Estimate: The ratio of carbon to hydrogen in the fuel by mass. The air/fuel ratio by Assume the percentage of nitrogen in air is: 76.7% by mass and 79% by volume (or mole).
Methane is burned completely with 25% excess air. Compute the number of moles of nitrogen in the products of combustion per mole of fuel. Use the editor to format your answer
Fuel oil has the following composition (in % by mass): carbon 85%, hydrogen 13%, and sulfur 2%. Calculate: (a) the stoichiometric and actual air-fuel ratios for the combustion with a 10% excess air in kg/kg, and (b) the mole fractions of the products of combustion. Ignore the air humidity.
A fuel consist of 84% Carbon, 13% Hydrogen, 2% Oxygen, and the remainder incombustible solid matter. Calculate the calorific value and the theoretical mass of air required per kg fuel and the mass analysis of the flue gas of 22kg of air are supplied per kg of fuel burned.
A gaseous fuel has he following composition by volume – CH4 = 25%, CO= 10%, H2= 6%, C3H8=10%. Calculate the weight of air required for complete combustion.
the full combustion is at constant pressure and the temperature of the products is (3250°C). Calculate 19.2/1) at 300° C. The internal energy of Ethane is equal (AU.= - 47590 kJ/mole) at (25 °C). when B) A cylinder contains a mixture of Ethane (C₂H) and air and the ratio of air to fuel is (A/F= the heat transferred from the combustion. Take specific heat: Reactants (C2H6-1.7, 02= 22.3, N2- 21.2 KJ/mole.K) Products (CO2= 46.5, H2O(Vap)= 27.3, 02-25.5 KJ/mole.K), R= 8.314 KJ/mole.K.
Octan fuel (C8H18) is burned with air in a combustion test, and a volumetric analysis reveals the following composition of the products: 11% CO₂ ; 3.6% 0 and 1.5% Co. Compute the actual air-fuel ratio used during the test and the 17.22, 1.15 Per cent theoretical air used. Ans

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