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Consider combustion of hydrogen gas in a mixture of hydrogen and oxygen adjacent to the metal wall of a combustion chamber. Combustion occurs at constant temperature and pressure according to the chemical reaction
(a) Determine an expression for and make a qualitative plot of
(b) Determine the value of
(c) On the same coordinates used in part (a), sketch curves for the concentrations of oxygen and water vapor.
(d) What is the molar flux of water vapor at
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Chapter 14 Solutions
Fundamentals of Heat and Mass Transfer
- Please answer fast I'll ratearrow_forwardA constant volume tank contain 1 mole of C7H14 and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C7H14 is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take AHo = -47800 kJ/kg).arrow_forwardButane (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?arrow_forward
- Using Hess' Law, calculate for the heat of combustion of a 1.5 liter propene (C3H6) at 14.5 psi and 80.6°F that is completely burned in air. Assume that all the water produced during the reaction is in liquid state. The standard enthalpy of formation of propene, C3H6 is +20.6 kJ/mol. The heats of formation of CO₂(g) and H₂O(l) are -394 kJ/mol and -285.8 kJ/, respectively.arrow_forwardButane (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?arrow_forwardYou are testing some novel fuel mixtures for potential use in automobiles. Your testing apparatus is a 2.54 cm inner diameter cylinder fitted with a piston, designed to mimic a cylinder found in a car engine. A fuel-air mixture is ignited while a force of F = 273.0 N is applied to the piston. There are 0.200 mol of gas after combustion at 290.0 °C, and the atmospheric pressure is 1.01325 x 105 Pa. Initial Final conditions conditions What is the pressure of gas inside the cylinder after combustion while a force of Fj = 273.0 N is applied to the cylinder? Assume combustion products behave ideally. 6.4 x105 Ра What is the volume of gas in the cylinder after combustion with a force of 273.0 N applied to the cylinder? 1.463 x10-3 V = m3 The force applied to the piston is then reduced to Ff = 111.0 N, and the gas responds in a two-step process. The first, quick step is adiabatic. During the second, slower step, the gas returns the change in kinetic and potential energies in both steps is…arrow_forward
- Wet air containing 4.0 mole% water vapor is passed through a column of calcium chloridepellets. The pellets adsorb 97.0% of the water and none of the other constituents of the air.The column packing was initially dry and had a mass of 3.40 kg. Following 5.0 hours ofoperation, the pellets are reweighed and found to have a mass of 3.54 kg. Calculate the molarflow rate (mol/h) of the feed gas and the mole fraction of water vapor in the product gas. Themole fraction of water in the product gas is monitored and found to have the value calculatedin part (a) for the first 10 hours of operation, but then it begins to increase.What is the most likely cause of the increase?If the process continues to run, what will the mole fraction of water in the product gaseventually be?arrow_forward1. The combustion of 1.00 mole of glucose, CeH12O6, tiberates 1.90 x 10 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 frøm 22.5 °C to 26.7 °C, what is the heat capacity of the calorirneter?arrow_forwardFuel 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.arrow_forward
- One mole of Carbon Dioxide burns completely in the presence of 3 moles of diatomic oxygen in a constant volume enclosure. The original temperature and pressure of the reactants are 25 C and 1 atm. A) If combustion takes place adiabatically calculate final temeprature and pressure of the products. B) If combustion does not take place adiabatically calculate the heat transfer per mole of CO when the products are cooled to a final temperature of 500K.arrow_forwardDetermine the adiabatic flame temperature (K) for a mixture of methane and 200% theoretical air that reacts completely in a steady-flow process at 1 atm. The methane and air enter the reaction at 298 K.arrow_forwardCalculate 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%arrow_forward
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