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]
Complete the balanced chemical equation for the combustion of methane, CH4. CH4 + 2 O2 + N 1 CO2 + H20 + q N2
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?
Calculate the minimum volume of air required for the complete combustion of 1 m³ of a gaseous fuel containing the following composition by volume: CO = 25%; H₂ = 10%; CH4 = 8%; CO₂ = 5%; N₂ = 50% and O₂ = 2%
Complete the balanced chemical equation for the combustion of methane, CH4. CH4 + O, + N2 → CO2 + H20 + N2
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
1. Determine the theoretical weight of air needed in kgair/kgfuel if the fuel used has 40.3°API. 2. A petrol has the following analysis: 85.5% carbon, 14.4% hydrogen, and 0.10% sulfur. Calculate the volume of air in m³ at 1.0 bar and 15°C required for perfect combustion of 1 kg of the fuel. 3. A typical industrial fuel oil, C16H32, is burned with 20% excess air. Calculate the actual weight of air in kgair/sec needed for 3.2 kg per sec of fuel. 4. A logging firm in Isabela operates a Diesel Electric plant to supply its electric energy requirements. During a 24-hour period, the plant consumed 350 gallons of fuel at 80 deg.F and produces 2700 kW-hrs. Industrial fuel used is 30°API and was purchased at P3.00 per liter at 60 deg.F. Determine the overall efficiency of the plant. 5. A diesel engine consumed 945 liters of fuel per day at 30°C. If the fuel was purchased at 15.5°C and 30°API at Php5.00/liter, determine the cost of fuel to operate the engine per day

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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.