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, H20(Vap)= 27.3, 02-25.5 KJ/mole.K), R= 8.314 KJ/mole.K.

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, H20(Vap)= 27.3, 02-25.5 KJ/mole.K), R= 8.314 KJ/mole.K.

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

See similar textbooks

Similar questions

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).
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]
Find the volume of the combustion products of 1 cu ft. Methane with 32% excess air at a pressure of 0.4 psi above atmospheric and a temperature of 1000 degree F.
1. A bituminous coal has the following composition as follows: C=71.5%, O=6%, S-4.6% W=3.4% H=5% N=1.3% Ash=3.2% Compute the amount of nitrogen produced during combustion process in lb/lb-coal. Also, determine the stoichiometric amount of air present in the combustion.
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]
The organic fuels methane and ethane has a volumetric analysis of 62% and 38%, respectively. If a complete combustion happens with 25% excess air, calculate for the theoretical total number of moles of water as a product of combustion.
The fuel supplied to a petrol engine is assumed to have the composition C10H22. If 42% excess air is supplied and combustion is complete . Calculate : 1- equivalence ratio. 2- The percentage volumetric.
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
3.1 Calculate the theoretical air/fuel and fuel/air ratios for the complete combustion of ethanol (C,H5OH). If the air is supplied at 1 bar and 25°C, calculate the volume of air required for complete combustion of fuel per kg and per kg mole of fuel.
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]
By analyzing the fuel, it was found that it consists of 85% carbon, 5% hydrogen, and 2% oxygen. 2% sulfur, percentages by weight, and the rest is nitrogen. Calculate the weight of the (standard) air required for each kilogram of fuel in order to complete combustion, and if the real air increases by 25%, calculate the percentage of dry products by weight and volume
There is a well-insulated open combustion chamber that ethane (C2H6) goes into at 77°F and 1 atm. The theoretical amount of air also enters at 220°F and 1 atm. The combustion is complete. Determine: a) The temperature of the combustion products coming out (°F)