Chapter 15: Problem 5
What does the dew-point temperature of the product gases represent? How is it determined?
Chapter 15: Problem 5
What does the dew-point temperature of the product gases represent? How is it determined?
All the tools & learning materials you need for study success - in one app.
Get started for freePropane gas \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) enters a steady-flow combustion chamber at 1 atm and \(25^{\circ} \mathrm{C}\) and is burned with air that enters the combustion chamber at the same state. Determine the adiabatic flame temperature for \((a)\) complete combustion with 100 percent theoretical air, ( \(b\) ) complete combustion with 200 percent theoretical air, and \((c)\) incomplete combustion (some \(\mathrm{CO}\) in the products) with 90 percent theoretical air.
Propane fuel (C \(_{3} \mathrm{H}_{8}\) ) is burned with stoichiometric amount of air in a water heater. The products of combustion are at 1 atm pressure and \(120^{\circ} \mathrm{F}\). What fraction of the water vapor in the products is vapor?
Octane gas \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) at \(25^{\circ} \mathrm{C}\) is burned steadily with 80 percent excess air at \(25^{\circ} \mathrm{C}, 1 \mathrm{atm},\) and 40 percent relative humidity. Assuming combustion is complete and the products leave the combustion chamber at \(1000 \mathrm{K}\), determine the heat transfer for this process per unit mass of octane.
Gaseous E10 fuel is 10 percent ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\right)\) and 90 percent octane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) on a kmol basis. This fuel is burned with 110 percent theoretical air. During the combustion process, 90 percent of the carbon in the fuel is converted to \(\mathrm{CO}_{2}\) and 10 percent is converted to CO. Determine \((a)\) the balanced combustion equation, (b) the dew-point temperature of the products, in \(^{\circ} \mathrm{C}\), for a product pressure of \(100 \mathrm{kPa}\) (c) the heat transfer for the process, in \(\mathrm{kJ}\), after \(2.5 \mathrm{kg}\) of fuel are burned and the reactants and products are at \(25^{\circ} \mathrm{C}\) with the water in the products remaining a gas, and (d) the relative humidity of atmospheric air for the case where the atmospheric air is at \(25^{\circ} \mathrm{C}\) and \(100 \mathrm{kPa}\) and the products are found to contain \(9.57 \mathrm{kmol}\) of water vapor per kmol of fuel burned.
Ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\) is burned with 175 percent theoretical air during a combustion process. Assuming complete combustion and a total pressure of 14.5 psia, determine (a) the air-fuel ratio and ( \(b\) ) the dew-point temperature of the products.
What do you think about this solution?
We value your feedback to improve our textbook solutions.