The volumetric analysis of the dry products of combustion of a hydrocarbon fuel describedby the general formula CxHy is: 13.6% CO₂ ; 0.4% 02; 0.8% Co; 0.4% CH4 and84.8% N₂ Determin the values of x and y for the fuel on the basis of 13.6 moles•of coz in the products of combustion.

Step 1:First write the balance equation for combustion of CxHyCxHy + (x + y/4)O2---> xCO2 +…

Answered: The volumetric analysis of the dry…

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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The products of combustion of an unknown hydrocarbon fuel C, H, have the following composition as measured by an Orsat apparatus: CO, 8.0%, CO 0.9%, 02 8.8% an N, 82.3%. Determine (a) the values of x and y, (b) the air fuel ratio, (c) the composition of the fuel, and (d) the percentage excess air used.
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]
Butane (C4H10) is completely combusted with air. All of the questions on this page refer to this process. Air contains 21% oxygen (O2) and 79% nitrogen (N2) on a molar basis. Element Symbol Molar Mass (kg/kmole) Hydrogen Carbon H. C 12 14 Nitrogen Oxygen 16 mair AF = mfuel % Excess Air = % of Theoretical (Stochiometric) Air - 100 % What is the air-fuel ratio (mass basis) at 200 % excess air?
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]
Butane (C4H10) is completely combusted with air. All of the questions on this page refer to this process. Air contains 21% oxygen (O2) and 79% nitrogen (N2) on a molar basis. Element Symbol Molar Mass (kg/kmole) Hydrogen Carbon C 12 14 Nitrogen Охуgen 16 mair AF = %3D Mfuel Excess Air = % of Theoretical (Stochiometric) Air - 100 % What is the air-fuel ratio (mass basis) at 200 % excess air?
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]
8. The combustion of 1.00 mole of glucose, C6H12O6, liberates 1.90 x 103 kJ of heat. If 2.30 g of glucose is burned in a calorimeter containing 0.560 kg of water, and the temperature of the assembly increases from 22.5 C to 26.7 C, what is the heat capacity of the calorimeter?
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
An analysis of the dry exhaust gas from an engine burning Benzole shows 15% Carbon Dioxide present by volume. The Benzole contains 90% C and 10% H₂ by mass. Assuming complete combustion, determine the air/fuel ratio used.
Aliquid fuel has a composition (by volume) C2H6 16% and CH4 84%. It is burned with theoretical amount of air required for stoichiometric mixture. Calculate the molecular weight 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%. ,
One Kmol of C8H18 is burned with 100% air containing 25 Kmol of O2. Determine the air-fuel ratio for this combustion process.
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.

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The volumetric analysis of the dry products of combustion of a hydrocarbon fuel described by the general formula CxHy is: 13.6% CO₂ ; 0.4% 02; 0.8% Co; 0.4% CH4 and 84.8% N₂ Determin the values of x and y for the fuel on the basis of 13.6 moles • of coz in the products of combustion.