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mechanical engineering

Thermodynamics An Engineering Approach 8th edition Yunus A. Cengel, Michael A. Boles - Solutions

Using EES (or other) software, determine the adiabatic flame temperature of the fuels CH4 (g), C2H2 (g), CH3OH (g), C3H8 (g), C8H18 (ℓ). Assume both the fuel and the airs enter the steady-flow combustion chamber at 25°C.
Using EES (or other) software, determine the minimum percent of excess air that needs to be used for the fuels CH4(g), C2H2(g), CH3OH(g), C3H8(g), C8H18(ℓ) if the adiabatic flame temperature is not to exceed 1500 K. Assume both the fuel and the air enter the steady flow combustion chamber at
Using EES (or other) software, repeat Prob.15–112 for adiabatic flame temperatures of (a) 1200 K, (b) 1750 K, and (c) 2000 K.
Using EES (or other) software, determine the adiabatic flame temperature of CH4(g) when both the fuel and the air enter the combustion chamber at 25°C for the cases of 0, 20, 40, 60, 80, 100, 200, 500, and 1000 percent excess air.
Using EES (or other) software, determine the rate of heat transfer for the fuels CH4 (g), C2H2 (g), CH3OH (g), C3H8 (g), and C8H18 (ℓ) when they are burned completely in a steady-flow combustion chamber with the theoretical amount of air. Assume the reactants enter the combustion chamber at
Using EES (or other) software, repeat Prob.15–115 for (a) 50, (b) 100, and (c) 200 percent excess air
Using EES (or other) software, determine the fuel among CH4 (g), C2H2 (g), C2H6 (g), C3H8 (g), C8H18 (ℓ) that gives the highest temperature when burned completely in an adiabatic constant-volume chamber with the theoretical amount of air. Assume the reactants are at the standard reference
A fuel is burned with 90 percent theoretical air. This is equivalent to (a) 10% excess air (b) 90% excess air (c) 10% deficiency of air (d) 90% deficiency of air (e) Stoichiometric amount of air
Propane (C3H8) is burned with 150 percent theoretical air. The air–fuel mass ratio for this combustion process is (a) 5.3 (b) 10.5 (c) 15.7 (d) 23.4 (e) 39.3
One kmol of methane (CH4) is burned with an unknown amount of air during a combustion process. If the combustion is complete and there are 2 kmol of free O2 in the products, the air–fuel mass ratio is (a) 34.3 (b) 17.2 (c) 19.0 (d) 14.9 (e) 12.1
A fuel is burned steadily in a combustion chamber. The combustion temperature will be the highest except when (a) The fuel is preheated. (b) The fuel is burned with a deficiency of air. (c) The air is dry. (d) The combustion chamber is well insulated. (e) The combustion is complete.
An equimolar mixture of carbon dioxide and water vapor at 1 atm and 60°C enter a dehumidifying section where the entire water vapor is condensed and removed from the mixture, and the carbon dioxide leaves at 1 atm and 60°C. The entropy change of carbon dioxide in the dehumidifying section is (a)
Methane (CH4) is burned completely with 80 percent excess air during a steady-flow combustion process. If both the reactants and the products are maintained at 25°C and 1 atm and the water in the products exists in the liquid form, the heat transfer from the combustion chamber per unit mass of
The higher heating value of a hydrocarbon fuel CnHm with m 8 is given to be 1560 MJ/kmol of fuel. Then its lower heating value is (a) 1384 MJ/kmol (b) 1208 MJ/kmol (c) 1402 MJ/kmol (d) 1514 MJ/kmol (e) 1551 MJ/kmol
Acetylene gas (C2H2) is burned completely during a steady-flow combustion process. The fuel and the air enter the combustion chamber at 25°C, and the products leave at 1500 K. If the enthalpy of the products relative to the standard reference state is 404 MJ/kmol of fuel, the heat transfer from
Benzene gas (C6H6) is burned with 90 percent theoretical air during a steady-flow combustion process. The mole fraction of the CO in the products is (a) 1.6% (b) 4.4% (c) 2.5% (d) 10% (e) 16.7%
A fuel is burned during a steady-flow combustion process. Heat is lost to the surroundings at 300 K at a rate of 1120 kW. The entropy of the reactants entering per unit time is 17 kW/K and that of the products is 15 kW/K. The total rate of energy destruction during this combustion process is (a)
Constant-volume vessels that contain flammable mixtures of hydrocarbon vapors and air at low pressures are frequently used. Although the ignition of such mixtures is very unlikely as there is no source of ignition in the tank, the Safety and Design Codes require that the tank withstand four times
Why is the criterion for chemical equilibrium expressed in terms of the Gibbs function instead of entropy?
Is a wooden table in chemical equilibrium with the air?
Write three different KP relations for reacting ideal gas mixtures, and state when each relation should be used.
The equilibrium constant of the reaction CO + ½O2 → CO2 at 1000 K and 1 atm is Kp1, Express the equilibrium constant of the following reactions at 1000 K in terms of Kp1: (a) CO + ½O2 CO2 at 3 atm (b) CO2 CO + 1/2 O2 at 1 atm (c) CO + O2 CO2 + ½ O2 at 1 atm (d) CO +
The equilibrium constant of the dissociation reaction H2 → 2H at 3000 K and 1 atm is Kp. Express the equilibrium constants of the following reactions at 3000 K in terms of Kp1. (a) H2 2H at 2 atm (b) 2H H2 at 1 atm (c) 2H2 4H at 1 atm (d) H2 + 2N2 2H + 2N2 at 2
Consider a mixture of CO2, CO, and O2 in equilibrium at a specified temperature and pressure. Now the pressure is doubled. (a) Will the equilibrium constant KP change? (b) Will the number of moles of CO2, CO, and O2 change? How?
Consider a mixture of CO2, CO, and O2 in equilibrium at a specified temperature and pressure. Now the pressure is doubled. (a) Will the equilibrium constant KP change? (b) Will the number of moles of CO2, CO, and O2 change? How? Discuss.
Consider a mixture of NO, O2, and N2 in equilibrium at a specified temperature and pressure. Now the pressure is tripled. (a) Will the equilibrium constant KP change? (b) Will the number of moles of NO, O2, and N2 change? How?
A reaction chamber contains a mixture of CO2, CO, and O2 in equilibrium at a specified temperature and pressure. How will (a) Increasing the temperature at constant pressure and (b) Increasing the pressure at constant temperature affect the number of moles of CO2?
A reaction chamber contains a mixture of N2 and N in equilibrium at a specified temperature and pressure. How will (a) increasing the temperature at constant pressure and (b) Increasing the pressure at constant temperature affect the number of moles of N2?
A reaction chamber contains a mixture of CO2, CO, and O2 in equilibrium at a specified temperature and pressure. Now some N2 is added to the mixture while the mixture temperature and pressure are kept constant. Will this affect the number of moles of O2? How?
Which element is more likely to dissociate into its monatomic form at 3000 K, H2 or N2? Why?
Using the Gibbs function data, determine the equilibrium constant KP for the reaction H2 + 1/2 O2 H2O at (a) 298 K and (b) 2000 K. Compare your results with the KP values listed in Table A–28.
Determine the equilibrium constant KP for the process CO + 1/2O2 = CO2 at (a) 298 K and (b) 2000 K. Compare your results with the values for KP listed in Table A–28.
Study the effect of varying the percent excess air during the steady-flow combustion of hydrogen at a pressure of 1 atm. At what temperature will 97 percent of H2 burn into H2O? Assume the equilibrium mixture consists of H2O, H2, O2, and N2.
Determine the equilibrium constant KP for the reaction CH4 + 2O2 CO2 + 2H2O at 25°C.
Using the Gibbs function data, determine the equilibrium constant KP for the dissociation process CO2 CO + 12 O2 at (a) 298 K and (b) 1800 K. Compare your results with the KP values listed in Table A–28.
Using the Gibbs function data, determine the equilibrium constant KP for the reaction at 25°C. Compare your result with the KP value listed in Table A–28.
Determine the temperature at which 5 percent of diatomic oxygen (O2) dissociates into monatomic oxygen (O) at a pressure of 3 atm.
Repeat Prob. 16–19 for a pressure of 6 atm.
Carbon monoxide is burned with 100 percent excess air during a steady-flow process at a pressure of 1 atm. At what temperature will 97 percent of CO burn to CO2? Assume the equilibrium mixture consists of CO2, CO, O2, and N2.
Reconsider Prob. 16–21. Using EES (or other) software, study the effect of varying the percent excess air during the steady-flow process from 0 to 200 percent on the temperature at which 97 percent of CO burns into CO2. Plot the temperature against the percent excess air, and discuss the results.
Repeat Prob. 16–21 using data in English units.
Hydrogen is burned with 150 percent theoretical air during a steady-flow process at a pressure of 1 atm. At what temperature will 98 percent of H2 burn to H2O? Assume the equilibrium mixture consists of H2O, H2, O2, and N2.
Air (79 percent N2 and 21 percent O2) is heated to 2000 K at a constant pressure of 2 atm. Assuming the equilibrium mixture consists of N2, O2, and NO, determine the equilibrium composition at this state. Is it realistic to assume that no monatomic oxygen or nitrogen will be present in the
Hydrogen (H2) is heated to 3200 K at a constant pressure of 8 atm. Determine the percentage of H2 that will dissociate into H during this process.
Carbon dioxide (CO2) is heated to 2400 K at a constant pressure of 3 atm. Determine the percentage of CO2 that will dissociate into CO and O2 during this process.
A mixture of 1 mol of CO and 3 mol of O2 is heated to 2200 K at a pressure of 2 atm. Determine the equilibrium composition, assuming the mixture consists of CO2, CO, and O2.
A mixture of 2 mol of CO, 2 mol of O2, and 6 mol of N2 is heated to 4320 R at a pressure of 3 atm. Determine the equilibrium composition of the mixture.
A mixture of 3 mol of N2, 1 mol of O2, and 0.1 mol of Ar is heated to 2400 K at a constant pressure of 10 atm. Assuming the equilibrium mixture consists of N2, O2, Ar, and NO, determine the equilibrium composition.
Determine the mole fraction of sodium that ionizes according to the reaction Na Na e- at 2000 K and 0.8 atm (KP + 0.668 for this reaction).
Liquid propane (C3H8) enters a combustion chamber at 25°C at a rate of 1.2 kg/min where it is mixed and burned with 150 percent excess air that enters the combustion chamber at 12°C. If the combustion gases consist of CO2, H2O, CO, O2, and N2 that exit at 1200 K and 2 atm, determine (a) the
Reconsider Prob. 16–32. Using EES (or other) software, investigate if it is realistic to disregard the presence of NO in the product gases?
A steady-flow combustion chamber is supplied with CO gas at 560 R and 16 psia at a rate of 12.5 ft3/min and with oxygen (O2) at 537 R and 16 psia at a rate of 0.7 lbm/min. The combustion products leave the combustion chamber at 3600 R and 16 psia. If the combustion gases consist of CO2, CO, and O2,
Oxygen (O2) is heated during a steady-flow process at 1 atm from 298 to 3000 K at a rate of 0.5 kg/min. Determine the rate of heat supply needed during this process, assuming (a) some O2 dissociates into O and (b) no dissociation takes place.
Estimate KP for the following equilibrium reaction at 2500 K CO + H2O = CO2 + H2 At 2000 K it is known that the enthalpy of reaction is -26176 kJ/kmol and KP is 0.2209. Compare your result with the value obtained from the definition of the equilibrium constant.
A constant-volume tank contains a mixture of 1 kmol H2 and 1 kmol O2 at 25°C and 1 atm. The contents are ignited. Determine the final temperature and pressure in the tank when the combustion gases are H2O, H2, and O2.
What is the equilibrium criterion for systems that involve two or more simultaneous chemical reactions?
When determining the equilibrium composition of a mixture involving simultaneous reactions, how would you determine the number of KP relations needed?
One mole of H2O is heated to 3400 K at a pressure of 1 atm. Determine the equilibrium composition, assuming that only H2O, OH, O2, and H2 are present.
A mixture of 2 mol of CO2 and 1 mol of O2 is heated to 3200 K at a pressure of 2 atm. Determine the equilibrium composition of the mixture, assuming that only CO2, CO, O2, and O are present.
Air (21 percent O2, 79 percent N2) is heated to 3000 K at a pressure of 2 atm. Determine the equilibrium composition, assuming that only O2, N2, O, and NO are present. Is it realistic to assume that no N will be present in the final equilibrium mixture?
Air (21 percent O2, 79 percent N2) is heated to 5400 R at a pressure of 1 atm. Determine the equilibrium composition, assuming that only O2, N2, O, and NO are present. Is it realistic to assume that no N will be present in the final equilibrium mixture?
Reconsider Prob. 16–43E Use EES (or other) software to obtain the equilibrium solution Compare your solution technique with that used in Prob. 16–43E.
Water vapor (H2O) is heated during a steady-flow process at 1 atm from 298 to 3000 K at a rate of 0.2 kg/min. Determine the rate of heat supply needed during this process, assuming (a) some H2O dissociates into H2, O2, and OH and (b) no dissociation takes place.
Reconsider Prob. 16–45. Using EES (or other) software, study the effect of the final temperature on the rate of heat supplied for the two cases. Let the final temperature vary from 2500 to 3500 K. For each of the two cases, plot the rate of heat supplied as a function final temperature.
Ethyl alcohol (C2H5OH(g)) at 25°C is burned in a steady-flow adiabatic combustion chamber with 40 percent excess air that also enters at 25°C. Determine the adiabatic flame temperature of the products at 1 atm assuming the significant equilibrium reactions are CO2 = CO + 1/2 O2 and 1/2 N2 + 1/2
Estimate the enthalpy of reaction hR for the combustion process of carbon monoxide at 2200 K, using (a) enthalpy data and (b) KP data.
Using the enthalpy of reaction hR data and the KP value at 2400 K, estimate the KP value of the combustion process H2 + 1/2O2 H2o at 2600 K
Estimate the enthalpy of reaction hR for the combustion process of carbon monoxide at 3960 R, using (a) Enthalpy data and (b) KP data.
Estimate the enthalpy of reaction hR for the dissociation process CO2 Co + 1/2O2 at 2200 K, using (a) enthalpy data and (b) Kp data.
Estimate the enthalpy of reaction hR for the dissociation process O2 2O at 3100K, using (a) enthalpy data and (b) Kp data.
Estimate the enthalpy of reaction for the equilibrium reaction CH4 + 2O2 = CO2 + 2H2O at 2500 K, using (a) Enthalpy data and (b) Kp data.
Consider a tank that contains a saturated liquid–vapor mixture of water in equilibrium. Some vapor is now allowed to escape the tank at constant temperature and pressure. Will this disturb the phase equilibrium and cause some of the liquid to evaporate?
Consider a two-phase mixture of ammonia and water in equilibrium. Can this mixture exist in two phases at the same temperature but at a different pressure?
Using the solubility data of a solid in a specified liquid, explain how you would determine the mole fraction of the solid in the liquid at the interface at a specified temperature.
Using solubility data of a gas in a solid, explain how you would determine the molar concentration of the gas in the solid at the solid–gas interface at a specified temperature.
Using the Henry’s constant data for a gas dissolved in a liquid explain how you would determine the mole fraction of the gas dissolved in the liquid at the interface at a specified temperature.
Show that a mixture of saturated liquid water and saturated water vapor at 100°C satisfies the criterion for phase equilibrium.
Show that a mixture of saturated liquid water and saturated water vapor at 300 kPa satisfies the criterion for phase equilibrium.
Show that a saturated liquid–vapor mixture of refrigerant- 134a at -10°C satisfies the criterion for phase equilibrium.
Consider a mixture of oxygen and nitrogen in the gas phase. How many independent properties are needed to fix the state of the system?
In absorption refrigeration systems, a two-phase equilibrium mixture of liquid ammonia (NH3) and water (H2O) is frequently used. Consider a liquid–vapor mixture of ammonia and water in equilibrium at 30°C. If the composition of the liquid phase is 60 percent NH3 and 40 percent H2O by mole
Consider a liquid–vapor mixture of ammonia and water in equilibrium at 25°C. If the composition of the liquid phase is 50 percent NH3 and 50 percent H2O by mole numbers, determine the composition of the vapor phase of this mixture. Saturation pressure of NH3 at 25°C is 1003.5 kPa.
A two-phase mixture of ammonia and water is in equilibrium at 50°C. If the composition of the vapor phase is 99 percent NH3 and 1 percent H2O by mole numbers, determine the composition of the liquid phase of this mixture. Saturation pressure of NH3 at 50°C is 2033.5 kPa.
Using the liquid–vapor equilibrium diagram of an oxygen–nitrogen mixture, determine the composition of each phase at 80 K and 100 kPa.
Using the liquid–vapor equilibrium diagram of an oxygen–nitrogen mixture, determine the composition of each phase at 84 K and 100 kPa.
Using the liquid–vapor equilibrium diagram of an oxygen–nitrogen mixture at 100 kPa, determine the temperature at which the composition of the vapor phase is 79 percent N2 and 21 percent O2.
Using the liquid–vapor equilibrium diagram of an oxygen–nitrogen mixture at 100 kPa, determine the temperature at which the composition of the liquid phase is 30 percent N2 and 70 percent O2.
Consider a rubber plate that is in contact with nitrogen gas at 298 K and 250 kPa. Determine the molar and mass density of nitrogen in the rubber at the interface.
A wall made of natural rubber separates O2 and N2 gases at 25°C and 500 kPa. Determine the molar concentrations of O2 and N2 in the wall.
Consider a glass of water in a room at 27°C and 97 kPa. If the relative humidity in the room is 100 percent and the water and the air are in thermal and phase equilibrium, determine (a) the mole fraction of the water vapor in the air and (b) the mole fraction of air in the water.
Water is sprayed into air at 80°F and 14.3 psia, and the falling water droplets are collected in a container on the floor. Determine the mass and mole fractions of air dissolved in the water.
Consider a carbonated drink in a bottle at 27°C and 130 kPa. Assuming the gas space above the liquid consists of a saturated mixture of CO2 and water vapor and treating the drink as water, determine (a) the mole fraction of the water vapor in the CO2 gas and (b) the mass of dissolved CO2 in a
Using the Gibbs function data, determine the equilibrium constant KP for the dissociation process O2 2O at 2000 K. Compare your result with the KP value listed in Table A–28.
A mixture of 1 mol of H2 and 1 mol of Ar is heated at a constant pressure of 1 atm until 15 percent of H2 dissociates into monatomic hydrogen (H). Determine the final temperature of the mixture.
A mixture of 1 mol of H2O, 2 mol of O2, and 5 mol of N2 is heated to 2200 K at a pressure of 5 atm. Assuming the equilibrium mixture consists of H2O, O2, N2, and H2, determine the equilibrium composition at this state. Is it realistic to assume that no OH will be present in the equilibrium mixture?
Determine the mole fraction of argon that ionizes according to the reaction Ar Ar+ + e- at 10,000 K and 0.35 atm (KP = 0.00042 for this reaction).
Methane gas (CH4) at 25°C is burned with the stoichiometric amount of air at 25°C during an adiabatic steady-flow combustion process at 1 atm. Assuming the product gases consist of CO2, H2O, CO, N2, and O2, determine (a) the equilibrium composition of the product gases and (b) the exit
Reconsider Prob. 16–81. Using EES (or other) software, study the effect of excess air on the equilibrium composition and the exit temperature by varying the percent excess air from 0 to 200 percent. Plot the exit temperature against the percent excess air, and discuss the results.
A constant-volume tank contains a mixture of 1 mol of H2 and 0.5 mol of O2 at 25°C and 1 atm. The contents of the tank are ignited, and the final temperature and pressure in the tank are 2800 K and 5 atm, respectively. If the combustion gases consist of H2O, H2, and O2, determine (a) the
A mixture of 2 mol of H2O and 3 mol of O2 is heated to 3600 K at a pressure of 8 atm. Determine the equilibrium composition of the mixture, assuming that only H2O, OH, O2, and H2 are present.

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